Answer and solve the following:

IV. Molecular formula

a. C₂H₂

b. C₂H₄

V. Emperical formula

a. C₅H₄

b. C₆H₆

VI. a. Reactants: Na₂SO₄(aq) + Ca(NO₃)₂(aq) Products: CaSO₄(s) + 2NaNO₃(aq) Type of reaction: Double displacement

b. Reactants: 3Mg(s) + N₂(g) Products: Mg₃N₂(s) Type of reaction: Combination

VII. a. 2Hg(NO₃)₂(s) → 2Hg(l) + 2NO₂(g) + O₂(g)

b. Ca₃(PO₄)₂(aq) + 2H₃PO₄(aq) → 3Ca(H₂PO₄)₂(aq)

c. 3NaOH(aq) + FeCl₃(aq) → Fe(OH)₃(s) + 3NaCl(aq)

A double displacement reaction, also known as a double replacement reaction or metathesis reaction, is a type of chemical reaction in which two compounds exchange or switch their constituent ions to form two new compounds.

In this type of reaction, the cations and anions of two ionic compounds exchange places to produce two new compounds, with no change in the oxidation state or charge of the elements involved. The general form of a double displacement reaction is AB + CD → AD + CB, where A, B, C, and D represent different ions or atoms.

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According to the periodical table's trends, an element with qualities like to sulfur (S) is most likely to mix with mag (Mg), as magnesium has a predisposition to react with sensitive nonmetals the same as sulfur and produce compounds.

For the majority of individuals, regular doses under 350 mg are safe. The adverse effects of magnesium can also include nausea, nausea, diarrhea, and upset stomach in some people. Magnesium is POSSIBLY SAFE Only if TAKEN IN VERY HIGH AMOUNTS (more than 350 mg daily).

And then use magnesium, individuals who have diabetes, digestive disease, heart disease, or renal disease should see their healthcare professional.

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The compounds formed are;

1) [tex]CrBr_{3}[/tex]

2) [tex]Fe_{2} O_{3}[/tex]

3)  [tex]((Hg)_2}) _{2} (CO_{3}) _{2}[/tex]

4) [tex]Ca(ClO_{3} )_{2}[/tex]

5)[tex](NH_{4}) _{3} PO_{4}[/tex]

Ionic compounds are formed through a type of chemical bonding called ionic bonding. Ionic bonding occurs when one or more electrons are transferred from one atom to another, resulting in the formation of ions, which are atoms or molecules that have a net electric charge due to a loss or gain of electrons.

The formation of ionic compounds typically occurs between atoms with large differences in electronegativity, or the ability of an atom to attract electrons.

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The pH at the equivalence point for the titration of 0.20 M HCl versus 0.10 M NaOH is 7.0.

The reaction between HCl and NaOH is a strong acid-strong base titration. At the equivalence point, all of the HCl has reacted with an equal amount of NaOH to form water and NaCl.

The balanced equation for the reaction is:

HCl + NaOH → NaCl + H2O

Since the reaction between HCl and NaOH is a 1:1 stoichiometric ratio, we can say that at the equivalence point, the moles of HCl consumed are equal to the moles of NaOH added.

Moles of HCl = concentration of HCl × volume of HCl used

Moles of NaOH = concentration of NaOH × volume of NaOH added

At the equivalence point, Moles of HCl = Moles of NaOH. Therefore,

concentration of HCl × volume of HCl used = concentration of NaOH × volume of NaOH added

Since we have equal volumes of HCl and NaOH at the equivalence point, we can simplify the equation to:

concentration of HCl = concentration of NaOH

Therefore, the concentration of HCl and NaOH at the equivalence point is both 0.15 M (the average of the initial concentrations of 0.20 M HCl and 0.10 M NaOH).

To find the pH at the equivalence point, we can use the equation for the dissociation of water:

H2O ⇌ H+ + OH-

At 25°C, the concentration of water is 55.5 M. At the equivalence point, the concentration of H+ and OH- are both equal, so we can write:

Kw = [H+][OH-]

where Kw is the ion product constant for water, which has a value of 1.0 × 10^-14 at 25°C.

At the equivalence point, the concentration of H+ and OH- are both equal to the concentration of NaOH and HCl, which is 0.15 M.

Therefore:

Kw = [H+][OH-]

1.0 × 10^-14 = [0.15][0.15]

[H+] = [OH-] = sqrt(1.0 × 10^-14) = 1.0 × 10^-7 M

The pH at the equivalence point is equal to the negative logarithm of the H+ concentration:

pH = -log[H+]

pH = -log(1.0 × 10^-7)

pH = 7.0

Therefore, the pH at the equivalence point for the titration of 0.20 M HCl versus 0.10 M NaOH is 7.0.

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Answer:

0.257383555 moles

Explanation:

The presence of water droplets on the cool upper portion of the test tube after heating the compound suggests that water molecules are trapped within its crystal structure. If the substance were a real hydrate, heating it would have caused all of the water molecules to evaporate, leaving behind an anhydrous substance.

What do you mean by crystalline compound?

The presence of water droplets on the cool upper portion of the test tube after heating the compound suggests that water molecules are trapped within its crystal structure. If the substance were a real hydrate, heating it would have caused all of the water molecules to evaporate, leaving behind an anhydrous substance.

However, the residue created a yellow-brown solution after being further dissolved in water, which is a certain sign of contaminants. When dissolved in water, true hydrates always produce a clear, colourless solution. Thus, the fact that the residue resulted in a coloured solution implies that the compound had impurities.

Together, the water stains and contaminants in the leftovers indicate that the original substance was not a genuine hydrate, but rather a mixture of the anhydrous substance and water, which may have been non-stoichiometrically trapped inside the crystal lattice or adsorbed onto the surface of the crystals.

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Answer:

the element is oxygen.

Explanation:

oxygen has six Valence electron which is why it's electron-dot structure also know as Lewis structure has six dots. it also has high electronegativity and form one-to-one bond with magnesium

Answer:

A

Refer to pic for explanation

Answer:

Explanation:

The balanced chemical equation for the reaction between magnesium carbonate and hydrochloric acid is:

MgCO3 + 2HCl → MgCl2 + H2O + CO2

From the equation, we can see that 1 mole of magnesium carbonate reacts with 2 moles of hydrochloric acid to produce 1 mole of carbon dioxide. The molar mass of magnesium carbonate is 84.3 g/mol, which means that 21 g of magnesium carbonate is equal to 0.25 moles (21/84.3). Therefore, 0.25 moles of magnesium carbonate will react with 0.5 moles of hydrochloric acid to produce 0.25 moles of carbon dioxide.

The volume of carbon dioxide can be calculated using the ideal gas law, which is 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. Assuming standard temperature and pressure (STP) of 273 K and 1 atm, we can use the molar volume of a gas at STP, which is 22.4 L/mol, to calculate the volume of carbon dioxide produced.

V = n × 22.4 L/mol

V = 0.25 mol × 22.4 L/mol

V = 5.6 L

Therefore, the volume of carbon dioxide produced when 21 g of magnesium carbonate reacts completely with excess hydrochloric acid is 5.6 L. The answer is option A, 4 dm³, which is approximately equal to 5.6 L.

When 43 g of ethyl lactate is burned in excess oxygen gas, 80.098 g of CO2 are formed.

What is Molecular Formula?

A molecular formula represents the actual number and type of atoms that make up a molecule of a compound. It shows the chemical symbols for the different elements in the compound and the subscript numbers that indicate the number of atoms of each element. For example, the molecular formula for water is H2O, which shows that each molecule of water contains two hydrogen atoms (H) and one oxygen atom (O).

First, we need to determine the molecular formula of ethyl lactate. The empirical formula of C5H10O3 has a molecular weight of approximately 118 g/mol (5 * 12.011 g/mol for carbon + 10 * 1.00794 g/mol for hydrogen + 3 * 15.9994 g/mol for oxygen).

To find the molecular formula, we need to know the actual molecular weight of ethyl lactate. We can use the given amount of ethyl lactate (43 g) to calculate the number of moles:

n = m/M = 43 g / 118 g/mol = 0.3644 mol

Now, we need to find the molecular formula. We can do this by dividing the molecular weight (118 g/mol) by the empirical formula weight (which we already calculated as 118 g/mol):

118 g/mol / 118 g/mol = 1

This tells us that the empirical formula is also the molecular formula, so ethyl lactate is C5H10O3.

Now we can use the balanced chemical equation for the combustion of ethyl lactate:

C5H10O3 + 8 O2 → 5 CO2 + 5 H2O

From the equation, we can see that 1 mol of ethyl lactate produces 5 mol of CO2. We already calculated that we have 0.3644 mol of ethyl lactate, so we can use this to find the amount of CO2 produced:

n(CO2) = 5 mol CO2/mol ethyl lactate * 0.3644 mol ethyl lactate = 1.822 mol CO2

Finally, we can convert this to grams of CO2:

m(CO2) = n(CO2) * M(CO2) = 1.822 mol * 44.0095 g/mol = 80.098 g

Therefore, when 43 g of ethyl lactate is burned in excess oxygen gas, 80.098 g of CO2 are formed.

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Answer:

The theoretical yield in moles of NH3 is 5.2 moles. This is calculated by dividing the mass of H2 (15.6 g) by the molar mass of H2 (2.016 g/mol) to get the number of moles of H2 (7.76 moles). Then, using the mole ratio from the balanced equation, we can calculate the number of moles of NH3 produced (5.2 moles).

Explanation:

Answer: C

Explanation: The assumption that pairing of electrons reduces orbital stability is not part of Bohr's theory.

Bohr's theory of atomic structure mainly focuses on the behavior of electrons in the atom and makes several key assumptions:

a) Energy is not dissipated when electrons move in an orbital (postulate of quantization)

b) Electrostatic force balances force tending to throw electron out of orbital (Coulomb's law)

d) Electrons move from one orbital to another by either absorbing or radiating energy (postulate of transitions)

Therefore, the correct answer is option (c) Pairing of electrons reduces orbital stability.

You use q = mcT again, but this time you assume qaluminum = qwater and solve for T, which is the ultimate temperature. You must research the specific heat values (c) of aluminum and water.

To calculate the heat capacity of a metal, use Q = smT. (In this calculation, make careful to include the heat given out by the metal, the mass of the metal, and the temperature change of the metal.)

The metal will cool and the water will heat up over time. The two things will eventually have the same temperature. They are then considered to be thermally balanced with one another.

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Stoichiometric amounts relate to the proportional amounts of reactants and products in a balanced chemical equation.

What transpires during a chemical reaction to the molecules of the reactants?

Only atoms from the reactants can wind up in the products of a chemical reaction. No atoms are annihilated or made into new ones. To create the products, the reactants come into contact with one another, the bonds between their atoms are broken, and the atoms then rearrange and establish new bonds.

The frequency of collisions between the two reactants will grow as the reactant concentration rises. There are times when collisions don't cause a response (atoms misaligned or insufficient energy, etc.). More collisions and reaction possibilities result from higher concentrations.

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Answer:

269.8

Explanation:

The balanced chemical equation for the reaction between aluminum and hydrochloric acid is:

2 Al + 6 HCl -> 2 AlCl3 + 3 H2

From the equation, we can see that 2 moles of aluminum react with 3 moles of H2 to produce 2 moles of AlCl3. Therefore, the molar ratio of aluminum to hydrogen gas is 2:3.

To find the mass of aluminum required to produce 30 grams of H2, we need to use the molar mass of hydrogen gas and the molar ratio between aluminum and hydrogen gas. The molar mass of hydrogen is approximately 1 g/mol.

First, we need to calculate the number of moles of hydrogen gas produced:

30 g H2 x (1 mol H2/2 g H2) = 15 mol H2

Since the molar ratio of aluminum to hydrogen gas is 2:3, we can calculate the number of moles of aluminum required:

15 mol H2 x (2 mol Al/3 mol H2) = 10 mol Al

Finally, we can calculate the mass of aluminum required:

10 mol Al x (26.98 g Al/mol) = 269.8 g Al

Therefore, approximately 269.8 grams of aluminum are required to produce 30 grams of H2.

The 8 anhydrοus salt has a mass οf 178 amu..

A mοle is the atοm's elementary particle, an iοn. The mοle οf the substance is always related tο the Avοgadrο number. The mοle is always assοciated with the weight οr mass οf the element οr substance. The standard unit οf a mοle is mοl. The mοle is a significant factοr οf the reactant and prοducts tο fοrm an equatiοn. A mοle calculates the atοm, iοn, and substance weighs.

The amοunt οf matter in a bοdy is referred tο as its mass. The kilοgrams is the kilοgrams, which is the SI unit οf mass (kg). Mass is defined as: Mass = Density /Vοlume.

mass οf water =45.1%    = 45.1 g

means that 45.1 g οf water in 100 g salt

hence mass οf anhydrοus salt(As)= 100 g  - 45.1 g =  54.9 g

mοlar mass οf anhydrοus salt (As) = 178 amu=178 g /mοl

mοlar mass οf water (H2O)=18.015 g /mοl

1st step:-     Find mοl οf  water

mοl οf water =   mass οf water /  mοlar mass οf water

=   45.1 g / 18.015 g /mοl

=  2.5035 mοl

2nd step:-      find mοl οf Anhydrοus salt

mοl οf  Anhydrοus salt (As) = mass οf anhydrοus salt /     mοlar mass οf anhydrοus salt

=     54.9 g  /  178 g /mοl

=  0.3084 mοl

3rd step:-calculate water οf crysatlisatiοn

=    mοl οf water  /   mοl οf  Anhydrοus salt    

=    2.5035 mοl /  0.3084

=  8.118  

=  8 (apprοx)

hence tοtal 8 mοl οf water present in Anhydrοus salt(As)   = As*8H20

Therefοre, 8 anhydrοus salt has a mass οf 178 amu.

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Diagram c to the left shows the repeating groups of atoms that make up the samples the chemist mixed together.

Atoms are the smallest unit of matter that make up all physical objects. Atoms are composed of three main components: protons, neutrons, and electrons. Protons and neutrons are found in the nucleus of the atom and have a positive charge, while electrons orbit the nucleus and have a negative charge. Atoms can join together to form molecules, which are the building blocks of all matter. Atoms of different elements can join together in different ways to form compounds and these compounds are the basis of all substances. Atoms are also the basis of all chemical reactions and can exist in different physical states, such as solid, liquid, or gas. Atoms can also be combined to form isotopes, which are atoms of the same element with different numbers of neutrons.

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The molecular formula of acetylene is C₂H₂ and ethylene is C₂H₄.

The simplest whole-number ratio of the atoms in a compound is shown by empirical formulae, the number of each type of atom in a molecule is shown by molecular formulas, and the bonds between the atoms in a molecule are shown by structural formulas. The empirical formula of naphthalene is C₁₀H₈ and benzene is C₆H₆.

The chemical formula of the reactants and products are:

The balanced reactions are:

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Rules Governing the Allowed Combinations of Quantum Numbers

The principal quantum range (n) can't be zero. The allowed values of n are consequently 1, 2, 3, 4, and so on. The angular quantum quantity (l) can be any integer between zero and n - 1. If n = 3, for example, l can be either 0, 1, or 2.

The set of quantum numbers n=1,l=1,ml=0,ms=+21 is no longer viable for an electron.

So right set of quantum numbers is n=2,l=1,m=0,s=+21.

Solution : The designation `4p` indicates that the orbital has a important quantum number `n = 4` and an angular-momentum quantum wide variety `l = 1`. The magnetic quantum quantity can have any of the values `-1, 0`, or `+1`.

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Answer: Oxygen and glucose are both reactants in the process of cellular respiration. The main product of cellular respiration

A Ph.D. or Psy.D. in psychology with a cognitive psychology concentration is normally required to be categorized as a cognitive psychologist. Thus, the choice is between a Ph.D. and a Psy.D.

False. While most cognitive psychologists do their study in academic institutions, some may work in governmental, nonprofit, or commercial organizations.

False. It is not compulsory to pursue a career in cognitive psychology, even though taking part in a Directed Independent Study (DIS) during your undergraduate studies may be advantageous to get research experience in the field. Other options for developing one's research abilities and experience include working in a lab or doing an internship.

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The rate of a reaction is proportional to the some power of the molar concentration of each of the reactants. The order gives us an idea about the kinetics of the reaction.

The order of a reaction is defined as the sum of the powers of the concentration terms of the reactants in the experimentally determined rate equation for the reaction. It is an experimental quantity.

a. The order of the alkene is 1

b. The order of the bromine s 2

c. The overall kinetic order is 3

Since the reaction is third order, the overall rate constant is mol²L⁻²s⁻¹ or M⁻²s⁻¹.

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Answer: None of the above

Explanation:

The dissolution can be sped up by stirring and it can be slowed by cooling the solution.

Breaking the solid into smaller pieces, grinding it into a powder, or using a solution with a larger surface area can increase the surface area of the solid, making it easier for the solvent to come into contact with the solid and dissolve it faster.

Stirring, shaking, or otherwise agitating the solution can help to increase the mixing of the solvent and the solid, which can speed up the dissolution process.

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18 moles of oxygen can be produced by decomposing 12 moles of KClO₃.

The balanced chemical equation for the decomposition of KClO₃ is:

2KClO₃ → 2KCl + 3O₂

According to the equation, for every 2 moles of KClO₃ decomposed, 3 moles of O₂ are produced. So, to determine how many moles of O₂ are produced by decomposing 12 moles of KClO₃, we can use the following proportion:

2 moles KClO₃ / 3 moles O₂ = 12 moles KClO₃ / x moles O₂

where x is the number of moles of O₂ produced.

Solving for x, we get:

x = (3 moles O₂)(12 moles KClO₃) / (2 moles KClO₃)

x = 18 moles O₂

Therefore, 12 moles of KClO₃ can produce 18 moles of O₂.

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The cation is mentioned first, followed by the anion, when identifying an ionic compound. Positive and negative charges must be equal. Certain anions with various forms are denoted by Roman numerals.

Ionic compounds, which are neutral substances, are made up of positively charged ions, known as cations, and negatively charged ions, known as anions. substances with binary ions (ionic compounds that contain only two types of elements).

The anion is written after the cation in the name. When a formula unit contains two or more of the same polyatomic ion, the subscript is written outside of the parenthesis.

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The empirical formula of decaborane is B5H7.

To find the empirical formula of decaborane, we need to determine the simplest whole-number ratio of atoms in the compound.

The molecular formula of decaborane is B10H14, which means it contains 10 boron atoms and 14 hydrogen atoms.

To determine the simplest ratio of boron to hydrogen atoms, we can divide each by the greatest common factor (GCF) of the two numbers.

The GCF of 10 and 14 is 2, so we divide each by 2:

B10H14 becomes B5H7

Therefore, the empirical formula of decaborane is B5H7 from B10H14

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