10. Solid HgO, liquid Hg, and gaseous O₂ are placed in a glass bulb and are allowed to reach equilibrium at a given temperature:

2HgO(s) 2Hg(1) + O₂(g)
Delta H = +43.4 kcal

The mass of HgO in the bulb could be increased by

a) removing some 0₂.
b) reducing the volume of the bulb.
c) increasing the temperature.
d) removing some Hg.

Answer: Your welcome!

Explanation:

Paragraph 1:

The atmosphere is composed of several layers, each with their own distinct characteristics. The closest layer to the earth is the troposphere which is about 10 miles above the surface of the earth. This layer is where we find most of our weather, temperature changes, and air pollution. The next layer is the stratosphere, which extends from 10 to 50 miles above the earth. This layer is known for its stable temperature and air pressure, as well as its concentration of ozone which absorbs much of the sun's ultraviolet radiation. At the top of the stratosphere is the mesosphere which extends to about 55 miles above the earth. This layer is known for its cold temperatures, making it the perfect place for meteoroids to burn up as they enter the atmosphere. Finally, the thermosphere extends from 55 to 400 miles above the earth, and is known for its extremely high temperatures, allowing for the aurora borealis to be visible here.

Paragraph 2:

To create a model of the atmosphere, one can use colored posterboard to represent the different layers. For example, the troposphere could be colored green to represent the air and clouds while the stratosphere could be colored blue to represent the ozone layer. The mesosphere could be colored orange to represent the burning of meteoroids, and the thermosphere could be colored purple to represent the aurora borealis. For each layer, one could provide a legend telling what each color represents, as well as a note about a special feature of each layer such as the activities that occur in each layer or the objects that can be seen in each layer. Additionally, one could provide the average temperature or temperature range of each layer, as well as how many miles from Earth each layer extends.

Paragraph 3:

Overall, creating a model of the atmosphere is an interesting and educational activity. By representing each layer in a different color, one can learn more about the different characteristics of each layer and how they relate to one another. Additionally, by providing a legend and notes about special features of each layer, one can gain a better understanding of the atmosphere and its components. Through this model, one can gain a better appreciation of the atmosphere and how it functions to protect our planet.

The balanced equation for the following chemical reactions are:

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 chemical reaction is balanced when the number of atoms of each element in the reactants equals the number of atoms of that element in the products. In other words, the law of conservation of mass is satisfied.

This means that no atoms are created or destroyed during a chemical reaction, they are only rearranged to form different molecules. To balance a chemical equation, coefficients are added in front of the chemical formulas to adjust the number of atoms of each element.

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The  likely statement that would be a result of switching from geothermal energy to biomass energy as the primary energy source for a home is

Deforestation would give way to land for crops.

Option C is correct.

Deforestation is described as the removal of a forest or stand of trees from land that is then converted to non-forest use.

Switching from geothermal energy to biomass energy would result to increase the demand for organic materials, leading to deforestation and a loss of habitat for wildlife.

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Hexane, heptane, and octane have molar masses of Hexane (C6H14) has a molecular mass of 6 (12.01 g/mol) and 14 (1.00 g/mol) and heptane (C7H16) has a molecular mass of 7 (12.01 g/mol) and 16 (1.00 g/mol) and 100.21 g/mol.

The mass in grammes of one mole of a chemical is its molar mass.The quantity of atoms, molecules, and ions contained in a substance is measured in terms of moles. A mole of any substance contains 6.022 x 1023 molecules.

Use 100 g of the fuel mixture as an example. Then:

Hexane weight is 28.30 grammes.

15.75 g is the heptane mass.

Octane mass is equal to 100 g, 28.30 g, 15.75 g, and 55.95 g.

The molar masses of hexane, heptane, and octane are:

Molar mass of hexane (C6H14) = 6(12.01 g/mol) + 14(1.01 g/mol) = 86.18 g/mol

Molar mass of heptane (C7H16) = 7(12.01 g/mol) + 16(1.01 g/mol) = 100.21 g/mol

Molar mass of octane (C8H18) = 8(12.01 g/mol) + 18(1.01 g/mol) = 114.23 g/mol

The number of moles of each component in 100 g of the fuel mixture is:

Moles of hexane = 28.30 g / 86.18 g/mol = 0.3282 mol

Moles of heptane = 15.75 g / 100.21 g/mol = 0.1573 mol

Moles of octane = 55.95 g / 114.23 g/mol = 0.4899 mol

Therefore, the mole fractions of each component are:

Mole fraction of hexane = 0.3282 / (0.3282 + 0.1573 + 0.4899) = 0.3841

Mole fraction of heptane = 0.1573 / (0.3282 + 0.1573 + 0.4899) = 0.1838

Mole fraction of octane = 0.4899 / (0.3282 + 0.1573 + 0.4899) = 0.4321

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The limiting reactant in this reaction is lead nitrate Pb(NO₃)₂. The mass of lead nitrate in this reaction is 331.2 g. The percent yield of PbI₂ is 76.5%.

The percent yield of a reaction is the ratio of its actual yield to the  theoretical yield multiplied by 100.

The limiting reactant of a reaction is the reactant which is not in sufficient quantity and as soon as it is consumed, the reaction stopes.

As per the given balanced equation, 2 moles of KI reacts with one mole of  lead nitrate. Then, 2.8 moles of KI need 1.4 moles of lead nitrate. Hence, Pb(NO₃)₂ is the limiting reactant.

molar mass of Pb(NO₃)₂ = 331.2 g/mol

molar mass of KI = 166 g/mol

mass of 2 moles = 332 g

mass of PbI₂ = 461 g/mol

mass of 0.765 moles = 352.6 g.

molar mass of KNO₃ = 101 g

mass of 1.53 moles = 154 .5 g.

One mole of Pb(NO₃)₂ gives one mole of PbI₂. Hence the theoretical yield is one mole. But the actual yield of the product lead iodide is 0.765 moles.

then percent yield = 0.765/1 × 100 = 76.5 %.

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A physical change is when a substance's phase changes. Low molecular attraction material C requires more energy to be moved out, which means its kinetic energy must be reduced.

Neither creation nor destruction of energy is possible. Yet, it is transferable from one type to another, preserving the system's overall energy.

In the liquid state, molecules or atoms have medium molecular affinity and are somewhat closer together than they are in the gaseous state, where they are widely apart and have low intermolecular forces of attraction.

As a material transforms from a gas to a liquid, its molecules condense and become closer to one another, creating a stronger molecular attraction.

Gas B has a medium level of molecular attraction, making it easy to liquify with little energy transfer, whereas gas C has a lower level of molecular attraction but a greater level of kinetic energy, requiring more energy transfer.

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When you increase the amount of carbon dioxide in the atmosphere, you also increase the amount of carbonic acid in the ocean.

Carbon dioxide is absorbed from the atmosphere into the ocean through a process called "oceanic uptake," which is facilitated by the exchange of gases at the air-sea interface.

As more carbon dioxide is emitted into the atmosphere, the concentration of carbon dioxide in the ocean increases, leading to a phenomenon called "ocean acidification".

Ocean acidification can have a number of negative impacts on marine organisms, including reduced growth rates and weakened shells or skeletons.

Thus, we can conclude this increases the amount of carbonic acid in ocean.

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The limiting reagent is chlorine.

The amount of excess reagent that will remain is 0.918 g of Al.

The balanced chemical equation for the reaction is:

2Al + 3Cl2 → 2AlCl3

The molar mass of Al is 26.98 g/mol and the molar mass of Cl2 is 70.90 g/mol. We can use these values to calculate the number of moles of each reactant:

moles of Al = 2.70 g / 26.98 g/mol = 0.100 mol

moles of Cl2 = 4.05 g / 70.90 g/mol = 0.057 mol

According to the balanced equation, 2 moles of Al react with 3 moles of Cl2 to produce 2 moles of AlCl3. Therefore, the amount of AlCl3 produced by each reactant is:

Al: (0.100 mol Al) x (2 mol AlCl3 / 2 mol Al) = 0.100 mol AlCl3

Cl2: (0.057 mol Cl2) x (2 mol AlCl3 / 3 mol Cl2) = 0.038 mol AlCl3

Since Cl2 produces less AlCl3, it is the limiting reagent. The amount of excess Al can be calculated as follows:

moles of excess Al = moles of Al - (moles of Cl2 x (2 mol Al / 3 mol Cl2))

moles of excess Al = 0.100 mol - (0.057 mol x (2/3))

moles of excess Al = 0.034 mol

The mass of excess Al can then be calculated using its molar mass:

mass of excess Al = moles of excess Al x molar mass of Al

mass of excess Al = 0.034 mol x 26.98 g/mol

mass of excess Al = 0.918 g

Therefore, 0.918 g of Al remains unreacted.

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Answer:

The relative formula mass of H₂O can be calculated by adding the atomic masses of two hydrogen atoms and one oxygen atom in the molecule. The atomic mass of hydrogen is 1 and the atomic mass of oxygen is 16. So, the relative formula mass of H₂O is:

(2 x 1) + 16 = 18

Explanation:

Answer:

NaCl

Explanation:

Therefore, the pressure when the container is expanded to 10.6 L is 367 mmHg.

Molarity, also known as molar concentration, is a unit of measurement used to express the concentration of a solution. It is defined as the number of moles of a solute dissolved in one liter of solution. The unit of molarity is moles per liter (mol/L), also written as M. For example, a solution with a molarity of 0.1 M contains 0.1 moles of solute per liter of solution. Molarity is commonly used in chemistry and biochemistry to describe the concentration of solutions in experiments and industrial processes.

Here,

We can use the combined gas law to solve for the new pressure:

P1V1/T1 = P2V2/T2

We are given:

P1 = 845 mmHg

V1 = 4.60 L

V2 = 10.6 L

Assuming that the temperature is constant, we can simplify the equation to:

P1V1 = P2V2

Solving for P2, we get:

P2 = P1V1/V2

Plugging in the values, we get:

P2 = 845 mmHg × 4.60 L / 10.6 L

P2 = 367 mmHg

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Answer:

The rearrangement of atoms is a chemical change.

Explanation:

Answer:

The net ionic equation of 2H+ + SO2 + Ca²+ + 2I → CaSO4 + 2H+ + 2I is C. H+ + SO4²+ Ca²+ + 2I→CaSO4+H*+ I. This equation describes the process of a single replacement reaction, where the hydrogen ions and iodide ions react with the sulfate and calcium ions to form the insoluble compound of calcium sulfate and the remaining hydrogen and iodide ions

Explanation:

The number of moles of A remaining at the new equilibrium is 1.93 mol.

Partial pressure is the pressure exerted by a single gas component in a mixture of gases, assuming that the other gas components are absent or ideal. In other words, it is the pressure that the gas would exert if it were the only gas in the container at the same volume and temperature.

In a mixture of gases, each gas contributes to the total pressure of the system, which is the sum of the partial pressures of each gas. This is meant to refer to as Dalton's law of partial pressures. The partial pressure of a gas is proportional to its mole fraction in the mixture, which is the ratio of the number of moles of the gas to the total number of moles of all gases in the mixture.

The balanced equation for the reaction is:

A(s) ⇌ B(g) + C(g)

Let's denote the initial amount of A as nA. Since the molar mass of A is not given, we cannot determine its mass directly from the number of moles. However, we know that the initial amount of A is 5.40 moles, so we can write:

nA = 5.40 mol

At equilibrium, the concentration of B is given as 1.40 M. Using the ideal gas law, we can relate the concentration of B to its partial pressure:

PV = nRT

where P is the partial pressure of B, V is the volume of the container, n is the number of moles of B, R is the gas constant, and T is the temperature. Assuming that the volume of the container does not change during the reaction, we can write:

P = nBRT/V

where nB equals the number of moles of B. Since the concentration of B is given as 1.40 M, we have:

nB/V = [B] = 1.40 M

Substituting into the previous equation, we obtain:

P = nBRT/V = (1.40 M)(R)(T)

At equilibrium, the partial pressures of B and C must be equal, so we have:

P = PB = PC

Let's denote the number of moles of B and C as nB and nC, respectively. Since the total number of moles in the system is conserved, we have:

nA = nB + nC

At equilibrium, the number of moles of B is equal to the number of moles of C, so we have:

nB = nC = 0.5(nA)

Substituting into the ideal gas law expression for P, we obtain:

P = PB = PC = nBRT/V = (0.5nA)(R)(T)/V

We can use this equation to calculate the value of P at equilibrium. Then, when the volume of the container is doubled, the new pressure will be:

P' = P/2

At the new equilibrium, the partial pressures of B and C must be equal, so we have:

P' = PB' = PC'

We can use the same logic as before to write:

PB' = PC' = (0.5nA')(R)(T)/(2V)

where nA' is the number of moles of A remaining at the new equilibrium. Setting PB' equal to P' and solving for nA', we obtain:

nA' = nA(P')/(2P) = (5.40 mol)(1/2)/(P/P') = (5.40 mol)(1/2)/(1.40/2) = 1.93 mol

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Precipitation reactions;

2KCl + Pb(NO3)2 ----> PbCl2 + 2KNO3

Ba(NO3)2 + K2SO4 -----> BaSO4 + 2KNO3

Hg2(C2H3O2)2 + 2NaCl -----> Hg2Cl2 + 2NaC2H3O2

Non precipitation reactions

C + O2 ---> CO2

HBr + KOH ----> KBr + H2O

HCl + KOH -----> KCl + H2O

H2O2 + NaOBr ----> NaBr + H2O + O2

A precipitation reaction is a type of chemical reaction that occurs when two aqueous solutions (solutions dissolved in water) are mixed together and form an insoluble solid called a precipitate.

The reaction is characterized by the exchange of ions between the two aqueous solutions, which leads to the formation of the insoluble solid.

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Fluorine is most likely the diatomic element with the mass of 19.08 grammes held in a container at 100°C (F2).

Diatomic molecules are those that contain two atoms. Iodine (I2), fluorine (F2), chlorine (Cl2), bromine (Br2), nitrogen (N2), oxygen (O2), and hydrogen (H2) are all diatomic elements. Diatomic molecules make up the bromine atom, Br2, in the periodic table.

The diatomic molecules of the group 7 elements are present. They have the chemical formulas F2, Cl2, Br2, and I2. Although the forces of attraction between molecules are minimal, the connection between the atoms in a molecule is quite strong. This explains why the boiling points of group 7 elements are low.

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Question:

Which of the following diatomic elements would have a mass of 19.08 grams stored in a container at and 100°C? (R= 0.0821 L atm/ mol K).

Thediatomic element with a mass of 19.08 grams stored in a container at 100°C is hydrogen (H2), which has a pressure of 27.2 atm.

What is Diatomic Elements?

Diatomic elements are chemical elements that exist as two atoms bound together in a molecule. Examples of diatomic elements include oxygen (O2), nitrogen (N2), hydrogen (H2), fluorine (F2), chlorine (Cl2), and iodine (I2).

To determine the diatomic element with a mass of 19.08 grams stored in a container at 100°C, we need to use the ideal gas law, which is given by:

PV = nRT

where P is the pressure of the gas, V is its volume, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature in Kelvin.

We can rearrange this equation to solve for the number of moles:

n = PV/RT

We are given the mass of the gas, which we can convert to moles using the molar mass of the element. The molar mass of a diatomic element is simply twice the atomic mass of the element. Using the periodic table, we find the following atomic masses:

H: 1.008

N: 14.007

O: 15.999

F: 18.998

We can calculate the molar mass of each diatomic element:

H2: 2 x 1.008 = 2.016 g/mol

N2: 2 x 14.007 = 28.014 g/mol

O2: 2 x 15.999 = 31.998 g/mol

F2: 2 x 18.998 = 37.996 g/mol

Now we can calculate the number of moles of the gas using the given mass and molar mass:

n = 19.08 g / molar mass

Using the molar masses above, we get:

For H2: n = 19.08 g / 2.016 g/mol = 9.47 mol

For N2: n = 19.08 g / 28.014 g/mol = 0.68 mol

For O2: n = 19.08 g / 31.998 g/mol = 0.60 mol

For F2: n = 19.08 g / 37.996 g/mol = 0.50 mol

Finally, we can use the ideal gas law to calculate the pressure of the gas, assuming a volume of 1 liter:

P = nRT/V = (number of moles) x R x (temperature in Kelvin) / V

Plugging in the values, we get:

For H2: P = 9.47 mol x 0.0821 L atm/mol K x (100+273.15) K / 1 L = 27.2 atm

For N2: P = 0.68 mol x 0.0821 L atm/mol K x (100+273.15) K / 1 L = 1.97 atm

For O2: P = 0.60 mol x 0.0821 L atm/mol K x (100+273.15) K / 1 L = 1.74 atm

For F2: P = 0.50 mol x 0.0821 L atm/mol K x (100+273.15) K / 1 L = 1.45 atm

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The initial concentration is 1.8 * 10^36 M.

The stoichiometry is 2A ⇒ B

The rate of disappearance of H2O2 is 4 mol/min

It decreases adhesion and increases cohesion

Not predictable since it can be at any level.

In a decomposition reaction, a single reactant breaks down into two or more products. The order of a decomposition reaction depends on the rate at which the reaction occurs with respect to the concentration of the reactant.

Given that;

ln[A] = ln[A]o - kt

ln(0.0015) = ln[A]o - (0.025 * 60 * 60)

-6.5 = ln[A]o - 90

-6.5 + 90 = ln[A]o

83.5 = ln[A]o

[A]o = e^83.5

[A]o = 1.8 * 10^36 M

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Between genes A and B, there is a wider separation or distance than between genes C and D.

The chance of recombination is 50% when the genes are distant from one another or on different chromosomes. In this instance, the two loci's allele inheritance is independent. Recombination frequency less than 50% indicates a connection between the two loci.

A illness that is passed from parent to kid may be linked to one or more genes with certainty thanks to genetic mapping. Moreover, mapping can reveal which chromosome a gene is located on and where exactly it is located on that chromosome.

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Molecular formula mass = empirical formula mass x n

We know that the molecular formula mass is approximately 60 g/mol, so that we can set up an equation:

60 g/mol = 30 g/mol x n

Solving for "n," we get:

n = 2

This means that the molecular formula of the compound is twice the empirical formula of C2H4O2. Therefore, the compound is acetic acid.

Acetic acid is one of the simplest carboxylic acids and is an important chemical reagent and industrial chemical. It is widely used in the production of vinyl acetate monomer (VAM), which is used in manufacturing polymers, adhesives, and coatings. It is also used as a solvent and preservative in food and other products.

Ethanoic acid is the main component of vinegar, typically a 5% solution of acetic acid in water. In addition to its industrial and commercial uses, acetic acid also has some medical applications, such as in treating ear infections and as a topical antimicrobial agent.

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Answer:

Explanation: K+ has a higher ionisation energy than Ca+ , so K has a higher second ionisation energy than Ca .

Answer:

D

Explanation:

Transfer of electrons from Na to Cl

Na has configuration of 2,8,1 it will lose one electron to Cl with configuration of 2,7 inorder for both to attain an octet configuration

Any time a liquid loses or receives energy, the temperature of the liquid changes.To calculate the amount pf energy change, the calorimeter monitors the weight of the fluid as well as the temperature change.

The 6000 series calorimeters' control systems serve as the foundation for the 6772 Calorimetric Thermometer, a high precision temperatures measuring device.It is a crucial component of both the 6755 Solution Calorimeter and the 6725 Semi-micro Calorimeter.

The calorimeter is a piece of equipment used in calorimetry, a procedure for calculating heat capacity and measuring the temperature of chemical processes or other physical changes.Among the most popular kinds are differential scanning operating, thermal micro cathode rays, titration calorimeters, and accelerated rate calorimeters.

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There are approximately 1.39 × 10²³ oxygen molecules in the balloon.

Oxygen is colorless, odorless and tasteless gas and it supports life. It is noncombustible but actively supports the burning of combustible materials.

To calculate number of oxygen molecules in the balloon, we use the Avogadro's number, which is equal to 6.022 × 10²³ molecules per mole of substance.

As moles of oxygen gas = mass of oxygen gas / molar mass of oxygen gas

moles of oxygen gas = 7.36 g / 32 g/mol

So, moles of oxygen gas = 0.23 mol

Now we use the Avogadro's number to calculate number of oxygen molecules in the balloon:

As number of oxygen molecules = moles of oxygen gas × Avogadro's number

number of oxygen molecules = 0.23 mol × 6.022 × 10²³  molecules/mol

number of oxygen molecules = 1.39 × 10²³  molecules

Therefore, there are approximately 1.39 × 10²³  oxygen molecules in the balloon.

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The percentage composition of magnesium hydroxide in the substance (Mg(OH)2) is 41.67%.

Magnesium hydroxide (Mg(OH)2) is of one magnesium (Mg) atom and two hydroxides (OH) ions.

The atomic mass of Mg = 24.31 g/mol

the atomic mass of O and H = 15.99 g/mol & 1.01 g/mol

The molecular weight of Mg(OH)2 is:

Mg(OH)2 = (24.31 g/mol) + 2(15.99 g/mol + 1.01 g/mol)

= 58.32 g/mol

To calculate percentage composition, we need to calculate the mass of magnesium in one molecule of  (Mg(OH)2)

Mass of Mg = 24.31 g/mol

The percentage composition of magnesium in Mg(OH)2 is:

(24.31 g/mol / 58.32 g/mol) x 100% ≈ 41.67%

Therefore, the percentage composition of magnesium in Mg(OH)2 is approximately 41.67%.

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The algorithm can be used to determine a wave's frequency if its wavelength is known: Frequency ⇒ 1/wavelength.

Define wavelength.

The extent of a wave is expressed by its wavelength. The wavelength is the distance between one wave's peak and the next wave's crest. The wavelength can also be determined by measuring from the "trough" (bottom) of one wave to the "trough" of the following wave.

Wavelength and frequency are inversely related. The number of waves that pass a fixed location in a unit of time is referred to as frequency. It also explains how many cycles or vibrations a body in periodic motion experiences in a given unit of time.

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No, using hydrochloric acid (HCl) to dissolve copper metal in the Preparation of Copper (I) Chloride experiment is not recommended because it would result in the formation of copper (II) chloride rather than copper (I) chloride.

How to prepare Copper (l) Chloride?

Copper metal reacts with hydrochloric acid to form copper (II) chloride and hydrogen gas:

Cu (s) + 2HCl (aq)

→ CuCl2 (aq) + H2 (g)

In contrast, when copper metal reacts with nitric acid, it is oxidized to copper (II) ions by the nitric acid. These copper (II) ions then react with copper metal to form copper (I) ions, which react with chloride ions to form copper (I) chloride:

Cu (s) + 4HNO3 (aq) → Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l)

Cu(NO3)2 (aq) + 2Cu (s) → 3Cu2+ (aq) + 2NO3- (aq)

3Cu2+ (aq) + 2Cl- (aq) → Cu3Cl2 (s)

Therefore, to obtain copper (I) chloride, it is necessary to use nitric acid in the first reaction.

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3.011  × 10²³ molecules are in 0.5 moles of PCl₃.

The mole is an amount unit similar to familiar units like pair, dozen, gross, etc. It provides a specific measure of the number of atoms or molecules in a bulk sample of matter.

A mole is defined as the amount of substance containing the same number of atoms, molecules, ions, etc. as the number of atoms in a sample of pure 12C weighing exactly 12 g.

Given,

Moles of PCl₃ = 0.5 moles

We know that 1 mole = 6.023 × 10²³ molecules

Thus, 0.5 moles will have 6.023 × 10²³ × 0.5 molecules.

= 3.011  × 10²³ molecules

Therefore, 3.011  × 10²³ molecules are in 0.5 moles of PCl₃.

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Answer:

First, we need to calculate the amount of heat required to raise the temperature of ice from -21°C to 0°C:

q1 = m × C_solid × ΔT = 31 g × 2.09 J/g·°C × (0°C - (-21°C)) = 1341.09 J

Next, we need to calculate the amount of heat required to melt the ice at 0°C:

q2 = m × ΔH_fusion = 31 g × 334 J/g = 10354 J

Then, we need to calculate the amount of heat required to raise the temperature of the liquid water from 0°C to 42°C:

q3 = m × C_liquid × ΔT = 31 g × 4.18 J/g·°C × (42°C - 0°C) = 5201.56 J

Finally, we need to calculate the amount of heat required to vaporize the liquid water at 100°C:

q4 = m × ΔH_vaporization = 31 g × 2260 J/g = 70060 J

The total amount of heat required is the sum of all four steps:

q_total = q1 + q2 + q3 + q4 = 86857.65 J

Converting to kJ:

q_total = 86.85765 kJ

Therefore, the amount of heat required to convert 31 g of ice at -21°C to liquid water at 42°C is approximately 86.9 kJ.

Explanation: