When magnesium reacts with hydrochloric acid, magnesium chloride and hydrogen gas are produced according to the balanced chemical equation. The amount of reactants and products can be calculated using stoichiometry.
What is Mole?
In chemistry, mole is a unit of measurement used to express amounts of a chemical substance. One mole of a substance contains the same number of entities, such as atoms, molecules, or ions, as there are in 12 grams of carbon-12.
a. The products of the reaction between Mg(s) and HCl(aq) are MgCl2(aq) and H2(g).
b. The balanced chemical equation is: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
c. In the reaction, solid magnesium (Mg) reacts with hydrochloric acid (HCl) to produce magnesium chloride (MgCl2) in solution and hydrogen gas (H2). The sentence equation for the reaction is: Magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen gas.
d. The balanced equation shows that 1 mole of Mg reacts with 2 moles of HCl. Therefore, if 1.54 moles of Mg reacts, it will consume 2 x 1.54 = 3.08 moles of HCl.
e. The balanced equation shows that 1 mole of HCl produces 1 mole of H2 gas. Therefore, 2.56 x 10(-7) grams of HCl will produce (1/36.46) x (2.56 x 10(-7)/1000) moles of H2 gas, which is approximately 7.01 x 10(-12) moles of H2 gas.
f. The balanced equation shows that 1 mole of Mg reacts with 2 moles of HCl. Therefore, to react with 0.03 moles of HCl, we need (0.03/2) moles of Mg, which is 0.015 moles of Mg. The mass of Mg needed can be calculated by multiplying the number of moles by the molar mass of Mg: 0.015 x 24.31 g/mol = 0.365 g of Mg.
g. The balanced equation shows that 1 mole of Mg produces 1 mole of H2 gas. Therefore, to produce 7.92 grams of H2 gas, we need (7.92/2) moles of Mg, which is 0.206 moles of Mg. The mass of Mg needed can be calculated by multiplying the number of moles by the molar mass of Mg: 0.206 x 24.31 g/mol = 5.00 g of Mg.
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In terms of chemical bonding, explain the difference in the rate of sugar & acid reaction to the reaction between KI(aq) and Pb(NO₃)₂(aq)
The difference in the rate of sugar and acid reaction to the reaction between KI(aq) and Pb(NO₃)₂(aq) can be explained by the type of chemical bonding present in each case. In the case of sugar and acid, the reaction is a covalent bond breaking and forming process that occurs gradually and can take time to complete.
Covalent bonds are relatively strong and require more energy to break, which can result in slower reaction rates.
On the other hand, the reaction between KI(aq) and Pb(NO₃)₂(aq) involves the formation and breaking of ionic bonds. Ionic bonds are relatively weaker than covalent bonds and require less energy to break, resulting in faster reaction rates.
Additionally, the presence of water in the reaction between KI(aq) and Pb(NO₃)₂(aq) can also speed up the reaction by facilitating the movement of ions and increasing their collision frequency.
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You are given 7. 69x10^23 molecules of HNO3. How many liters do you
have?
Pls help
Answer:
7.3
Explanation:
Ideal Gas Law --
PV=nRT
Standard Conditions these are listed on the back of the periodic table slightly different-look now
Pressure: 1 atm = 760 mmHg = 760 torr = 101.3 kPa
Temperature : 273 K = 0°C
To convert from °C to K add 273 to the °C temperature
To convert back to °C subtract 273 from the Kelvin temperature
*Reminder: R = 0.0821 L atm/mol K so volume must be in liters, pressure must be in atm, amount
mol K must be in moles NOT GRAMS, and temperature must be in kelvin
1. How many moles of gas are contained in 890.0 mL at 21.0 °C and 750.0 mm Hg pressure?
2. 1.09 g of H, is contained in a 2.00 L container at 20.0 °C. What is the pressure in this container?
3. Calculate the volume 3.00 moles of a gas will occupy at 24.0 °C and 762.4 mm Hg.
4. What volume will 20.0 g of Argon occupy at STP?
5. How many moles of gas would be present in a gas trapped within a 100.0 mL vessel at 25.0 °C
at a pressure of 2.50 atmospheres?
6. How many moles of a gas would be present in a gas trapped within a 37.0 liter vessel at 80.00
°C at a pressure of 2.50 atm?
7. If the number of moles of a gas is doubled, at the same temperature and pressure, will the volume increase or decrease?
8. What volume will 1.27 moles of helium gas occupy at STP?
9. At what pressure would 0.150 mole of nitrogen gas at 23.0 °C occupy 8.90 L?
10. What volume would 32.0 g of NO, gas occupy at 3.12 atm and 18.0 °C?
1. The number of moles that are contained in 890 ml at 21.0 °C and 750.0 mm Hg pressure is 0.0368 moles
The ideal gas law states
PV = nRT
where P is the pressure
V is the volume
n is the number of moles
R is the gas constant
T is the temperature
Given:
P = 760 mmHg
760 mmHg = 1 atm
P = 1 atm
T = 21° C = 21+273 K = 294 K
V = 890 ml = 0.89 L
Putting them in ideal gas law,
1 * 0.89 = n * 0.0821 * 294
n = 0.0368
2. The pressure of the container containing 1.09 g of H in a 2.00 L container at 20.0 °C is 6.55 atm
V = 2 L
n = 1.09/2 = 0.545
T = 20 + 273 K = 293 K
Putting them in ideal gas law,
P * 2 = 0.545 * 0.0821 * 293
P = 6.55 atm
3. The volume of 3.00 moles of gas will occupy at 24.0 °C and 762.4 mm Hg is 72.93 L
P = 762.4 mmHg
P = 1.003 atm
n = 3 moles
T = 24 + 273 K = 297 K
Putting them in ideal gas law,
V * 1.003 = 3 * 0.0821 * 297
V = 72.93 L
4. The volume of 20 g of Argon at STP is 11.2 L
P = 1 atm
T = 273 K
n = 20/40 = 0.5
Putting them in ideal gas law,
V * 1 = 0.5 * 0.0821 * 273
V = 11.2 L
5. The number of moles of gas that would be present in a gas trapped within a 100.0 mL vessel at 25.0 °C is 0.01
V = 100 ml = 0.1 L
T = 25 + 273 = 298 K
P = 2.5 atm
Thus, 2.5 * 0.1 = n * 0.0821 * 298
n = 0.01
6. The moles of gas that would be present in a gas trapped within a 37.0-liter vessel at 80.00 °C at a pressure of 2.50 atm is 3.19 moles
P = 2.5 atm
T = 80 + 273 K = 353 K
V = 37 L
Thus, 2.5 * 37 = 0.0821 * n * 353
n = 3.19
7. The volume will increase if the number of moles of a gas is doubled, at the same temperature and pressure
Keeping the temperature and pressure constant in the gas law we get,
V ∝ n
Thus, the volume is directly proportional to number of moles in this case.
8. The volume occupied by 1.27 moles of helium gas at STP is 28.46 L
P = 1 atm
T = 273 K
n = 1.27
Putting them in ideal gas law,
V * 1 = 1.27 * 0.0821 * 273
V = 28.46 L
9. At pressure 0.415 atm, 0.150 moles of nitrogen gas at 23.0 °C occupy 8.90 L
V = 8.9 L
T = 23 + 273 K = 300 K
n = 0.15 moles
Thus, P * 8.9 = 0.0821 * 0.15 * 300
P = 0.415 atm
10. The volume occupied by 32g of NO at 3.12 atm and 18.0 °C is 8.11 L
n = 32/30 = 1.06
P = 3.12 atm
T = 273 + 18 K = 291 K
Thus, 3.12 * V = 1.06 * 0.0821 * 291
V = 8.11 L
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D. When the astronauts get this water in space they perform electrolysis and only are able to
experimentally make 43,200g of O₂. Using this as your experimental (actual) yield and your answer
from part C as your theoretical, calculate the percent yield of Oxygen.
actual yield
theoretical yield
x 100%
percent yield
=
Answer:
The theoretical yield of oxygen (O2) can be calculated using the balanced chemical equation:
2 H2O(l) → 2 H2(g) + O2(g)
From part (c), we calculated that 90.0 g of water (H2O) can produce 31.98 g of oxygen (O2). Therefore, the theoretical yield of oxygen from 43,200 g of water is:
theoretical yield = (31.98 g O2 / 90.0 g H2O) x 43,200 g H2O
theoretical yield = 15,379.2 g O2
The percent yield of oxygen can be calculated using the formula:
percent yield = (actual yield / theoretical yield) x 100%
Substituting the given values, we get:
percent yield = (43,200 g / 15,379.2 g) x 100%
percent yield ≈ 280.9%
This result seems unusually high, and suggests an error in the calculations or experimental data. A percent yield greater than 100% indicates that the actual yield is greater than the theoretical yield, which is usually not possible due to limitations in the reaction conditions or experimental procedures.
how many moles of aluminum oxide AI2O3 can you produce if you have two moles of AI
How many grams of magnesium can be heated to raise the temperature 45 C and absorb 843 J of energy
Explanation:
You will need the specific heat of Mg which I found to be 1.02 J / (g C)
m * 45 C * 1.02 J . (g C) = 843
m = 843 / (45* 1.02) = 18.4 g of Magnesium
The solubility of Ag,PO, in water at 25 °C is 4.3 x10-5 M. What is Ksp for Ag3PO? A) 2.1 x 10-12 B) 1.8 x 109 C) 9.2 × 10-17 D) 3.1 × 10-17
The solubility of Ag and PO, in water at 25 °C is 4.3 x10-5 M. The Ksp for Ag3PO is 2.1 x 10-12. Thus, option A) is correct.
Solubility refers to the maximum amount of a substance that can dissolve in a given solvent at a certain temperature and pressure. In this case, Ag3PO4 has a solubility of 4.3 x 10-5 M in water at 25°C. The Ksp (solubility product constant) for Ag3PO4 can be calculated using the following equation:
Ag3PO4(s) ⇌ 3Ag+(aq) + PO43-(aq)
Ksp = [Ag+]3 [PO43-]
To calculate Ksp, we need to determine the concentration of Ag+ and PO43- ions in solution. Since Ag3PO4 dissociates into three Ag+ ions and one PO43- ion, the concentration of Ag+ ions will be three times the solubility of Ag3PO4:
[Ag+] = 3(4.3 x 10-5 M) = 1.29 x 10-4 M
The concentration of PO43- ions will be equal to the solubility of Ag3PO4:
[PO43-] = 4.3 x 10-5 M
Now, we can plug these concentrations into the Ksp equation:
Ksp = (1.29 x 10-4)3 (4.3 x 10-5) = 2.1 x 10-12
Therefore, the answer is A) 2.1 x 10-12.
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Dry ice (above) is made from carbon dioxide gas at extremely low temperatures and very high pressures. A 0.25 g sample of dry ice contains molecules CO2:
Answer:To find the number of CO2 molecules in a 0.25 g sample of dry ice, we can use the Avogadro's number and the molar mass of CO2.The molar mass of CO2 is:12.01 g/mol (C) + 2(16.00 g/mol) (O) = 44.01 g/molThis means that 1 mole of CO2 contains 6.022 x 10^23 molecules.To find the number of moles in 0.25 g of CO2, we can use the molar mass:0.25 g / 44.01 g/mol = 0.005681 molFinally, we can use Avogadro's number to find the number of CO2 molecules:0.005681 mol x 6.022 x 10^23 molecules/mol = 3.422 x 10^21 CO2 moleculesTherefore, a 0.25 g sample of dry ice contains approximately 3.422 x 10^21 CO2 molecules.
What volume of 0. 018 M H2SO4 is needed to contain 97 g of H2SO4
To prepare 97 g of H₂SO₄, 45.3 liters of 0.018 M H₂SO₄ solution would be required.
To calculate the volume of 0.018 M H₂SO₄ needed to contain 97 g of H₂SO₄, we first need to determine the number of moles of H₂SO₄ in 97 g. From the molar mass of H₂SO₄, we can calculate that 97 g is equivalent to 0.815 moles of H₂SO₄ .
Using the molarity of the H₂SO₄ solution (0.018 M), we can then calculate the volume of solution needed using the formula:
Volume = moles / molarity
Thus, the volume of 0.018 M H₂SO₄ needed to contain 97 g of H₂SO₄ is:
Volume = 0.815 moles / 0.018 M = 45.3 L (rounded to two decimal places).
Therefore, 45.3 liters of 0.018 M H₂SO₄ solution would be needed to contain 97 g of H₂SO₄.
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What is the molarity of a solution if 1. 75 moles of KOH are dissolved in 2. 5 liters of water а 39 М с 0. 70 М b. 1А М d 4. 4M А В ОООО
To calculate the molarity of a solution, we need to know the number of moles of solute and the volume of the solution in liters.
a. 39 M solution with 0.70 M KOH:
Number of moles of KOH = 0.70 moles/Liter x 2.5 Liters = 1.75 moles
Volume of solution = 2.5 Liters
Molarity of solution = Number of moles of solute / Volume of solution = 1.75 moles / 2.5 Liters = 0.70 M
b. 1 A solution:
This question is incomplete, as it is not specified what solute is dissolved in the solution. Therefore, it is not possible to calculate the molarity of the solution without this information.
c. 4.4 M solution of ABOOOO:
It is not possible to calculate the molarity of this solution without more information about the solute dissolved in the solution. The chemical formula or name of the solute is needed to determine the number of moles present in the solution.
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A 0.205g sample of caco3 is added to a flask with 7.50ml of 2.00 m hcl.
caco3(aq)+2hcl(aq)-cacl2(aq) + h2o(l) + co2
enough water is added to make a 125.0ml solution.a 10.00ml aliquot of this solution is taken and titred with 0.058 naoh
naoh (aq) + hcl - h2o + nacl
how many ml of naoh are used?
The volume of [tex]NaOH[/tex] used to titrate the[tex]HCl[/tex] is 5.80 mL
First, we need to find the number of moles of [tex]HCl[/tex] that reacted with the [tex]CaCO3[/tex].
2 mol [tex]HCl[/tex] react with 1 mol [tex]CaCO3[/tex]
Moles of [tex]HCl[/tex] = (7.50 mL) x (2.00 mol/L) = 0.015 mol [tex]HCl[/tex]
From the balanced equation, we see that 1 mol of [tex]CaCO3[/tex] reacts with 2 mol of [tex]HCl[/tex]. Therefore, the number of moles of [tex]CaCO3[/tex] in the original 0.205 g sample is:
Moles of[tex]CaCO3[/tex] = 0.205 g / 100.09 g/mol = 0.002049 mol [tex]CaCO3[/tex]
Since 1 mol of [tex]CaCO3[/tex] produces 1 mol of [tex]CO2[/tex], we have:
Moles of[tex]CO2[/tex]produced = 0.002049 mol [tex]CaCO3[/tex]
Now we need to calculate the concentration of [tex]CO2[/tex] in the final 125.0 mL solution.
Concentration of [tex]CO2[/tex] = Moles of [tex]CO2[/tex] produced / Volume of solution
Concentration of [tex]CO2[/tex] = 0.002049 mol / 0.125 L = 0.0164 mol/L
Finally, we can use the balanced equation for the titration reaction to calculate the number of moles of [tex]NaOH[/tex]used.
1 mol [tex]NaOH[/tex] reacts with 1 mol [tex]HCl[/tex]
Moles of [tex]NaOH[/tex] used = (0.058 L) x (0.1000 mol/L) = 0.0058 mol [tex]NaOH[/tex]
Since the volume of the aliquot is 10.00 mL or 0.0100 L, the concentration of [tex]HCl[/tex] is:
Concentration of [tex]HCl[/tex] = Moles of NaOH used / Volume of [tex]HCl[/tex]
Concentration of [tex]HCl[/tex] = 0.0058 mol / 0.0100 L = 0.580 M
Therefore, the volume of [tex]NaOH[/tex] used to titrate the [tex]HCl[/tex]is:
Volume of [tex]NaOH[/tex] = (0.580 M) x (0.0100 L) = 0.00580 L or 5.80 mL
So, the answer is 5.80 mL.
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Calculate the volume of 2. 30 moles of gas exerting a pressure of 2. 80 atm at 155°C.
The volume of 2. 30 moles of gas exerting a pressure of 2. 80 atm at 155°C is 84.7 L.
We can use the ideal gas law to solve for the volume:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature to Kelvin:
155°C + 273.15 = 428.15 K
Next, we can plug in the values and solve for V:
V = (nRT) / P
V = (2.30 mol * 0.08206 Latm/molK * 428.15 K) / 2.80 atm
V = 84.7 L
Therefore, the volume of 2.30 moles of gas exerting a pressure of 2.80 atm at 155°C is 84.7 L.
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A rock contains one-fourth of its original amount of potassium-40. The half life of potasium-40 is 1. 3 billion years. Calculate the rock´s age
The age of the rock is approximately 2.6 billion years.
The fact that the rock contains one-fourth of its original amount of potassium-40 means that three-quarters of the original potassium-40 has decayed.
Since the half-life of potassium-40 is 1.3 billion years, this means that the rock has gone through two half-lives of decay.
To calculate the age of the rock, we can use the following formula:
age = number of half-lives x half-life
In this case, the number of half-lives is 2 and the half-life is 1.3 billion years. Plugging these values into the formula, we get:
age = 2 x 1.3 billion years
age = 2.6 billion years
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If 66. 38 g of potassium chloride reacts with fluorine and produces potassium fluoride and chlorine how many moles of chlorine can you get?
When 66.38 g of potassium chloride reacts with fluorine, you can obtain 0.4452 moles of chlorine.
To find out how many moles of chlorine you can get when 66.38 g of potassium chloride reacts with fluorine to produce potassium fluoride and chlorine, you'll need to follow these steps:
1. Write the balanced chemical equation for the reaction:
2 KCl + F2 → 2 KF + Cl2
2. Determine the molar mass of KCl (potassium chloride):
39.10 g/mol (K) + 35.45 g/mol (Cl) = 74.55 g/mol
3. Convert the given mass of KCl (66.38 g) to moles:
(66.38 g KCl) / (74.55 g/mol) = 0.8904 mol KCl
4. Use the stoichiometry from the balanced equation to determine the moles of Cl2 (chlorine) produced:
(0.8904 mol KCl) x (1 mol Cl2 / 2 mol KCl) = 0.4452 mol Cl2
So, when 66.38 g of potassium chloride reacts with fluorine, you can obtain 0.4452 moles of chlorine.
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If a piece of metal at 150 *C is placed in a beaker with 50 ml water at 60*C.
a. What is likely to happen to the temperature of the water in the beaker?.
b. What is likely to happen to change with the metal?.
a) The temperature of the water in the beaker is likely to increase as heat flows from the metal to the water until they reach thermal equilibrium.
b) The metal will likely lose heat to the water until it reaches thermal equilibrium with the water.
a) The temperature of the water in the beaker is likely to increase due to the transfer of heat from the metal to the water. This process is known as conduction, and it occurs because heat always flows from hotter objects to cooler objects. The metal, being at a higher temperature than the water, will transfer heat to the water until both reach a state of thermal equilibrium.
b) The amount of heat lost by the metal will depend on its mass, specific heat capacity, and initial temperature. The metal may also undergo physical changes due to the change in temperature, such as contraction or expansion. The type of metal and its properties will influence how much it changes in response to the temperature change.
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How many moles of ch₃nh₃cl need to be added to 200.0 ml of a 0.500 m solution of ch₃nh₂ (kb for ch₃nh₂ is 4.4 × 10⁻⁴) to make a buffer with a ph of 11?
You need to add 0.405 moles of CH₃NH₃Cl to 200.0 mL of 0.500 M CH₃NH₂ to create a buffer with a pH of 11.
To find the moles of CH₃NH₃Cl needed, you'll need to use the Henderson-Hasselbalch equation and the given information.
The Henderson-Hasselbalch equation is pH = pKa + log([A⁻]/[HA]).
First, calculate pKa using the given Kb value for CH₃NH₂:
pKa = -log(Ka)
= -log(Kw/Kb)
= -log(1.0 × 10⁻¹⁴ / 4.4 × 10⁻⁴)
= 10.36.
Then, plug in the desired pH (11) and the given concentrations of CH₃NH₂ (0.500 M):
11 = 10.36 + log([CH₃NH₃Cl]/[0.500]).
Solving for [CH₃NH₃Cl], you get [CH₃NH₃Cl] = 0.405 M.
Finally, multiply this concentration by the volume of the solution in liters (0.200 L) to find the moles of CH₃NH₃Cl needed: 0.405 M × 0.200 L = 0.405 moles.
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How much 3. 0 M H2SO4 is needed to neutralize 50. ML of 1. 2 M AL(OH)3
The amount of H₂SO₄ needed is 30 mL, under the condition that the required amount is needed to neutralize 50. ML of 1. 2 M AL(OH)₃.
In order to solve this problem, we need to apply stoichiometry and the balanced chemical equation for the reaction between H₂SO₄ and AL(OH)₃.
The derived balanced chemical equation for this reaction is
2AL(OH)₃ + 3H₂SO₄ → Al₂(SO₄)₃ + 6H₂O
Now regarding the equation, we can evaluate that 3 moles of H₂SO₄ are necessary to react with 2 moles of AL(OH)₃.
We can apply this information to calculate how much H₂SO₄ is needed to neutralize 50 mL of 1.2 M AL(OH)₃.
Step 1, we need to calculate how many moles of AL(OH)₃ are present in 50 mL of 1.2 M solution:
Molarity = moles of solute / liters of solution
1.2 M = moles of AL(OH)₃ / 0.050 L
moles of AL(OH)₃ = 0.060 moles
Now we can apply stoichiometry to calculate how many moles of H₂SO₄ are required
moles of H₂SO₄ = (0.060 moles AL(OH)₃ x (3 moles H₂SO₄ / 2 moles AL(OH)₃
moles of H₂SO₄ = 0.090 moles
Finally, we can evaluate how many milliliters of 3.0 M H₂SO₄ are required
Molarity = moles of solute / liters of solution
3.0 M = 0.090 moles / liters of solution
liters of solution = 0.030 L
We need to convert liters to milliliters:
0.030 L x (1000 mL / 1 L)
= 30 mL
Hence, 30 mL of 3.0 M H₂SO₄ are necessary to neutralize 50 mL of 1.2 M AL(OH)₃.
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6
camryn will: attempt 1
question 15 (3 points)
a steam turbine has an efficiency of 40.0%. a steam engine has an efficiency of
25.0%. suppose both devices are provided with 1000 j of thermal energy. how much
more useful work will the steam turbine do? show your work.
pa..
в у
h.
Steam turbine will do 150 J more useful work
Given the efficiency of both a steam turbine (40.0%) and a steam engine (25.0%), we can calculate the amount of useful work each device can do when provided with 1000 J of thermal energy.
For the steam turbine:
Efficiency = (Useful work output) / (Input energy)
0.4 = (Useful work output) / (1000 J)
Useful work output = 0.4 * 1000 J = 400 J
For the steam engine:
Efficiency = (Useful work output) / (Input energy)
0.25 = (Useful work output) / (1000 J)
Useful work output = 0.25 * 1000 J = 250 J
Now, we can find the difference in useful work between the two devices:
Difference = Useful work (steam turbine) - Useful work (steam engine)
Difference = 400 J - 250 J = 150 J
So, the steam turbine will do 150 J more useful work than the steam engine when provided with 1000 J of thermal energy.
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PLEASE HELP FAST.
Perform the following
mathematical operation, and
report the answer to the
appropriate number of
significant figures.
1. 6524 + 5. 67 = [ ? ]
The answer to the appropriate number of significant figures is 6530.67.
Explanation:
When adding two numbers, the number of decimal places in the result should be the same as the number of decimal places in the number with the fewest decimal places. In this case, 6524 has no decimal places and 5.67 has two decimal places. Therefore, the answer should have two decimal places.
When adding whole numbers, the number of significant figures in the result should be the same as the number of significant figures in the number with the fewest significant figures. In this case, both numbers have four significant figures. Therefore, the answer should also have four significant figures.
Adding the two numbers gives:
6524
+ 5.67
-------
6530.67
Therefore, the answer to the appropriate number of significant figures is 6530.67.
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G Trehalose, C12H22O11, is a nonreducing sugar that is only 45% as sweet as sugar. When hydrolyzed by aqueous acid or an alpha-glucosidase, it forms only D-glucose. When it is treated with excess methyl iodide in the presence of Ag2O and then hydrolyzed with water under acidic conditions, only 2,3,4,6-tetra-O-methyl-D-glucose is formed. Complete the structure of trehalose
The structure of trehalose can be determined based on its chemical formula, [tex]C12H22O11[/tex], and the fact that it only forms D-glucose upon hydrolysis.
Trehalose is a disaccharide composed of two glucose molecules linked by an alpha-1,1 glycosidic bond. This means that the glucose molecules are joined together through their first and first carbon atoms, respectively. The structure can be written as:
[tex]HOCH2(CHOH)4α-D-Glc-(1→1)-α-D-Glc-CH2OH[/tex]
where [tex]"α-D-Glc"[/tex] represents a glucose molecule in its alpha configuration.
To visualize the structure, we can draw it in a condensed form, where the two glucose molecules are shown connected by a straight line:
[tex]HOCH2(CHOH)4α-D-Glc-(1→1)-α-D-Glc-CH2OH[/tex]
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Part B
One of the main components of an airbag is the gas that fills it. As part of the design process, you need to determine the exact amount of nitrogen that should be produced. Calculate the number of moles of nitrogen required to fill the airbag. Show your work. Assume that the nitrogen produced by the chemical reaction is at a temperature of 495°C and that nitrogen gas behaves like an ideal gas. Use this fact sheet to review the ideal gas law.
Part C
Recall the balanced chemical equation from part B of task 1:
2NaN3 → 2Na + 3N2.
Calculate the mass of sodium azide required to decompose and produce the number of moles of nitrogen you calculated in part B of this task. Refer to the periodic table to get the atomic weights
To calculate the number of moles of nitrogen required to fill the airbag, we need to use the ideal gas law.
We know the temperature of the nitrogen gas produced by the chemical reaction, which is 495°C, and we assume that it behaves like an ideal gas.
We also know the volume of the airbag, which we can use to calculate the number of moles of nitrogen using the ideal gas law equation PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.
Once we have calculated the number of moles of nitrogen required, we can move on to part C of the question, which asks us to calculate the mass of sodium azide required to produce that amount of nitrogen.
To do this, we need to refer to the balanced chemical equation given in part B and use the atomic weights from the periodic table to calculate the mass of sodium azide needed.
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Can acids neutralize bases?
Answer:
yes acid can nuetralize bases
Answer:
Yes!
Explanation:
Strong Acids neutralize Strong bases.
When they react, water is formed. Whatever ions are left over, they become salt.
There must be an equal moles of strong acid and strong base.
Gerald t. Moneybottom loves trees so much that he bought the entire amazon rain forest and fenced it off, preventing any logging. In doing so, he caused a number of valuable endangered tree species to be saved, resulting in new medicines being developed. It also resulted in a lot of carbon dioxide being absorbed, slowing global warming. Gerald t. Moneybottom is providing….
Gerald T. Moneybottom's action of buying the Amazon rainforest and protecting it from logging has significant positive impacts on both the environment and human health.
By preventing logging, he ensures the survival of various endangered tree species, which could have otherwise become extinct. The rainforest is home to many unique plants and animals that have yet to be discovered and studied, and some of these species could potentially have medicinal properties.
By protecting the rainforest, Moneybottom has provided an opportunity for scientists to study these species and develop new medicines that can improve human health.
In addition to the medicinal benefits, the rainforest also serves as a natural carbon sink, absorbing carbon dioxide from the atmosphere and slowing down the process of global warming.
The preservation of the Amazon rainforest helps to mitigate the effects of climate change by reducing the amount of carbon dioxide in the atmosphere. This action contributes to the effort to reduce greenhouse gas emissions and fight climate change, which is a critical global issue.
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Calculate the amount of electrical energy (in kWh) needed to produce
1.00E3 kg of aluminum using electrolysis if the applied voltage is 6.00 V. (1
kWh = 3.6E6 J)
The amount of electrical energy (in kWh) needed to produce 1 kWh of electrical energy is 1 kWh or 3.6E6 J. The actual amount of energy needed may vary depending on the efficiency of the power generation system used.
A kilowatt-hour is a unit of energy commonly used by electric companies to measure the amount of energy consumed by households or businesses over a period of time. One kilowatt-hour (kWh) is equal to the amount of energy consumed by a 1,000 watt appliance for one hour.
We know that 1 kWh is equal to 3.6E6 J (joules). This means that to produce 1 kWh of electrical energy, we need to generate 3.6E6 J of energy.
In practical terms, the amount of electrical energy needed to produce 1 kWh depends on the efficiency of the power generation system. For example, a coal-fired power plant may require more energy input (e.g. coal) to generate 1 kWh of electrical energy compared to a renewable energy source such as solar or wind power.
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How many magnesium ions are contained in 4.5 moles of magnesium phosphate?
8.13 x 10²⁴ magnesium ions in 4.5 moles of magnesium phosphate.
To determine the chemical formula for magnesium phosphate. Magnesium has a 2⁺ charge, and phosphate has a 3⁻ charge, so the chemical formula for magnesium phosphate is Mg₃(PO₄)₂.
Next, we need to use the coefficients in the formula to determine the number of magnesium ions in 4.5 moles of magnesium phosphate. There are 3 magnesium ions in one molecule of magnesium phosphate, so we can set up a proportion:
3 Mg ions / 1 Mg₃(PO₄)₂ molecule = x Mg ions / 4.5 moles Mg₃(PO₄)₂
Solving for x, we get:
x = 3 Mg ions / 1 Mg₃(PO₄)₂ molecule × 4.5 moles Mg₃(PO₄)₂
x = 13.5 moles Mg ions
Therefore, there are 13.5 moles of magnesium ions in 4.5 moles of magnesium phosphate. However, if we want to convert this to a more common unit, we can use Avogadro's number to convert moles to atoms or ions:
13.5 moles Mg ions × 6.022 x 10²³ions/mol = 8.13 x 10²⁴ Mg ions
Therefore, there are approximately 8.13 x 10²⁴ magnesium ions in 4.5 moles of magnesium phosphate.
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Given the chart of bond energies, calculate the enthalpy change for the reaction below. Show all work
The enthalpy of the reaction can be obtained as 118 kJ/mol.
What is the reaction enthalpy?Reaction enthalpy, also known as heat of reaction or ΔHrxn, is the change in enthalpy that occurs during a chemical reaction. It is defined as the difference between the enthalpy of the products and the enthalpy of the reactants.
We have;
Enthalpy of reaction = Bonds broken - Bonds formed
Enthalpy of reaction = [4(413) + 2(495) - [2(799) + 2(463)
= [1652 + 990] - [1598 + 926]
=2642 - 2524
= 118 kJ/mol
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0.97 g of product were generated in a reaction, which corresponds to 63.1% yield. what is the theoretical yield of this reaction in grams?
The theoretical yield of this reaction in grams is approximately 1.54 g.
The theoretical yield of a reaction is the maximum amount of product that could be obtained if the reaction went to completion. In this case, since we know the actual yield (0.97 g) and the percent yield (63.1%), we can use this information to calculate the theoretical yield.
First, we can use the percent yield formula to calculate the actual amount of product that was expected based on the theoretical yield:
Percent yield = (actual yield / theoretical yield) x 100
Rearranging this formula, we can solve for the theoretical yield:
Theoretical yield = actual yield / (percent yield / 100)
Plugging in the values we know, we get:
Theoretical yield = 0.97 g / (63.1 / 100) = 1.54 g
Therefore, the theoretical yield of this reaction is 1.54 g. This means that if the reaction had gone to completion, we would have expected to obtain 1.54 g of product. The actual yield of 0.97 g represents only 63.1% of the theoretical yield.
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50.0 g (convert mL to L) of water cools from 100°C to 88°C. What is the correct description of the heat transfer? The specific heat capacity of water is 4.184 J/g·°C. Use the equation q= m x C x T change. T change = Final temperature- Initial temperature.
Group of answer choices
600 joules are released
2510 joules are absorbed
600 joules are absorbed
2510 joules are released
The correct description of the heat transfer is heat is released. Hence the heat released is 2150 J (last option)
How do i determine the heat released?The following data were obtained from the question:
Mass of water (M) = 50.0 gInitial temperature of water (T₁) = 100 °CFinal temperature of water (T₂) = 88 °CChange in temperature (ΔT) = 88 - 100 = -12 °C Specific heat capacity of water (C) = 4.184 J/gºC Heat energy (Q) =?The heat released or absorbed can be obtain as follow:
Q = MCΔT
Q = 50 × 4.184 × -12
Q = -2510 J
From the above, we can see that the heat energy is negative (i.e -2510 J).
Thus, we can conclude that the description of the heat transfer is heat is released (last option)
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∆E = −33 kJ/mol Ea = 20 kJ/mol What is E a′ ?
Answer in units of kJ/mol.
The value of Ea′ is -53 kJ/mol, and it represents the energy released during the chemical reaction.
The given values ∆E = −33 kJ/mol and Ea = 20 kJ/mol represent the activation energy and the change in energy, respectively, for a chemical reaction. The activation energy, Ea, is the minimum energy required for the reaction to occur, while the change in energy, ∆E, represents the difference between the energy of the reactants and the energy of the products.
The relationship between the activation energy, Ea, and the change in energy, ∆E, can be expressed using the equation: ∆E = Ea + Ea′ where Ea′ represents the energy released during the reaction. Since the change in energy and the activation energy are given, we can rearrange the equation to solve for Ea′: Ea′ = ∆E - Ea
Substituting the given values, we get: Ea′ = −33 kJ/mol - 20 kJ/mol = -53 kJ/mol. Therefore, the value of Ea′ is -53 kJ/mol. This negative value indicates that the reaction is exothermic, meaning that it releases energy as it proceeds. The magnitude of the value (-53 kJ/mol) indicates that the energy released during the reaction is significant.
In summary, the value of Ea′ is -53 kJ/mol, and it represents the energy released during the chemical reaction. This value can be calculated using the equation Ea′ = ∆E - Ea, where ∆E is the change in energy and Ea is the activation energy.
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Coach pollard still thinks he is really fast and so he went out to sprint at the track meet. he ran at a velocity of 4 m/s. his mass is about 68 kg. about how much kinetic energy did coach pollard use before he inevitably hurt himself after the run? ke=1/2mv^2
Coach Pollard used about 544 J of kinetic energy during his sprint.
Kinetic energy is the energy possessed by a moving object due to its motion. In this case, Coach Pollard's kinetic energy is directly proportional to his mass and the square of his velocity. As he runs faster or has more mass, his kinetic energy will increase accordingly. This is important to consider in athletics and sports where energy and power are key factors in performance.
The kinetic energy of Coach Pollard can be calculated using the formula KE = 1/2mv², where m is the mass of Coach Pollard and v is his velocity. Substituting the given values, we get KE = 1/2 × 68 kg × (4 m/s)² = 1/2 × 68 kg × 16 m²/s² = 544 J. As a result, Coach Pollard used approximately 544 J of kinetic energy throughout his sprint.
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