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slega [8]
3 years ago
11

Find ΔHrxn for the following reaction: 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g)

Chemistry
1 answer:
ch4aika [34]3 years ago
5 0

Answer:

ΔH°rxn = -827.5 kJ

Explanation:

Let's consider the following balanced equation.

2 PbS(s) + 3 O₂(g) → 2 PbO(s) + 2 SO₂(g)

We can calculate the standard enthalpy of reaction (ΔH°rxn) from the standard enthalpies of formation (ΔH°f) using the following expression.

ΔH°rxn = [2 mol × ΔH°f(PbO(s)) + 2 mol × ΔH°f(SO₂(g) )] - [2 mol × ΔH°f(PbS(s)) + 3 mol × ΔH°f(O₂(g) )]

ΔH°rxn = [2 mol × ΔH°f(PbO(s)) + 2 mol × ΔH°f(SO₂(g) )] - [2 mol × ΔH°f(PbS(s)) + 3 mol × ΔH°f(O₂(g) )]

ΔH°rxn = [2 mol × (-217.32 kJ/mol) + 2 mol × (-296.83)] - [2 mol × (-100.4) + 3 mol × 0 kJ/mol]

ΔH°rxn = -827.5 kJ

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Calculate the new pressure of a gas if the gas at 50 ˚C and 81.0 kPa is heated to 100 ˚C at a constant volume.
Debora [2.8K]

Answer:

93.5 kPa

Explanation:

Step 1: Given data

  • Initial pressure (P₁): 81.0 kPa
  • Initial temperature (T₁): 50 °C
  • Final pressure (P₂): ?
  • Final volume (T₂): 100 °C

Step 2: Convert the temperatures to the Kelvin scale

When working with gases, we need to consider the absolute temperature. We will convert from Celsius to Kelvin using the following expression.

K = °C + 273.15

T₁: K = 50°C + 273.15 = 323 K

T₂: K = 100°C + 275.15 = 373 K

Step 3: Calculate the final pressure of the gas

At a constant volume, we can calculate the final pressure of the gas using Gay-Lussac's law.

P₁/T₁ = P₂/T₂

P₂ = P₁ × T₂/T₁

P₂ = 81.0 kPa × 373 K/323 K

P₂ = 93.5 kPa

7 0
3 years ago
Explain the Law of Conservation of Energy!
kaheart [24]
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5 0
3 years ago
Read 2 more answers
Determine the value of the equilibrium constant, Kgoal, for the reactionN2(g)+H2O(g)⇌NO(g)+12N2H4(g), Kgoal=?by making use of th
Black_prince [1.1K]

Answer:

K_{goal}=1.793*10^{-33}

Explanation:

N2(g)+O2(g)⇌2NO(g), K_1 = 4.10*10^{-31}

N2(g)+2H2(g)⇌N2H4(g), K_2 = 7.40*10^{-26}

2H2O(g)⇌2H2(g)+O2(g), K_3 = 1.06*10^{-10}

If we add above reaction we will get:

2N2(g)+2H2O(g)⇌2NO(g)+N2H4(g)                     Eq (1)

Equilibrium constant for Eq (1) is K_1*K_3*K_3

Divide Eq (1) by 2, it will become:

N2(g)+H2O(g)⇌NO(g)+1/2N2H4(g)                       Eq (2)  

Equilibrium constant for Eq (2) is (K_1*K_3*K_3)^{1/2}

Equilibrium constant =K_{goal}= (K_1*K_2*K_3)^{1/2}\\K_{goal}= (4.10*10^{-31} *7.40*10^{-26}*1.06*10^{-10})^{1/2}\\K_{goal}=1.793*10^{-33}

7 0
3 years ago
What is the molar mass of a gas if 0. 473 g of the gas occupies a volume of 376 ml at 23. 0°c and 1. 90 atm?.
frozen [14]

Answer:

The molecular weight of the unknown gas is 16.1 g/mol.

6 0
2 years ago
Determine whether each statement is an example of a physical change or a chemical change. Newspaper yellows in the sun. Physical
miss Akunina [59]

Answer:

the newspaper one is a chemical change because the chemicals in the paper have reacted with something and turned a different color. the wax one is a physical change because it is a change in the phase of matter, which is always a physical change (still the same substance chemically)

7 0
2 years ago
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