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Chapter 13 Problems

20 original chapter problems from Chemistry II, Chapter 5. Review quizzes remain in their original lessons.

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Carbon Dioxide can react with Hydrogen to form Methane. The reaction is as follows. Name three ways of pushing the equilibrium to the right.
$CO_{2(g)}+4H_{2(g)}\leftrightarrow CH_{4(g)}+2H_2O_{(g)}$

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Reviewed replacement: in a 1.00 L closed ideal-gas vessel at a fixed stated temperature, A(g)⇌B(g), K_c=12.4. Initially [A]=0.100 M and [B]=0. Calculate equilibrium [B].

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Reviewed replacement: in a constant-volume irreversible model, the methane partial-pressure disappearance law is −dp/dt=kp², with k=0.0422 (atm·s)⁻¹. How long does p fall from 0.400 atm to 0.200 atm?

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Ammonia is fixed from atmospheric nitrogen by reacting it with hydrogen. Given that the equilibrium constant is 2.7, if a greenhouse starts out at 1atm, with 70% Nitrogen and 0.5% Hydrogen, what will the partial pressure of ammonia be at equilibrium?

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Ammonia gas reacts with oxygen according to the following unbalanced equation. A reactor held at 10L and 25ºC contains 4mol of Ammonia and 5mol of Oxygen gas. What is the total pressure of the container at equilibrium?
$NH_{3(g)}+O_{2(g)}\leftrightarrow NO_{(g)}+H_2O_{(g)}$ $K = 2.22$

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Reviewed replacement: an irreversible first-order disappearance model for a gas has k=32.0 min⁻¹. How long does its partial pressure fall from 0.100 atm to 0.0100 atm at fixed volume and temperature?

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Hydrogen Cyanide gas can be produced by reacting Methane and Ammonia. The reaction has a $\Delta H=251 \frac {kJ}{mol}$ .
$CH_{4(g)}+NH_{3(g)}\leftrightarrow HCN_{(g)}+3H_{2(g)}$
The system is currently at equilibrium. Declare what happens under the following conditions:
a) System volume increases
b) Temperature increases
c) Pressure of Ammonia increases

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Reviewed replacement: A(aq)⇌B(aq) has K_c=7.231. An ideal 0.800 L solution initially has [A]=0.600 M and [B]=0. Calculate the moles of B at equilibrium.

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Elemental sulfur can be obtained by treating Hydrogen Sulfide gas with Sulfur Dioxide. If a 100L reactor chamber at 20ºC reacts with 10atm Hydrogen Sulfide and 7atm Sulfur Dioxide, how much Sulfur is created at equilibrium?
$2H_2S_{(g)}+SO_{2(g)}\leftrightarrow 3S_{(s)}+2H_2O_{(g)}$ $K = 0.843$

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In 1890, a way to purify Nickel was discovered. It involved passing heated Carbon Monoxide over Nickel. The two reacted to form Nickel Tetracarbonyl ( $Ni(CO)_4$ ) gas. at 50ºC, the equilibrium constant is 12.3. A container is initially at 100kPa CO and contains 10g of Nickel. The container is heated to 50ºC, and its volume is 5L. What is the equilibrium mass of Nickel in the container?

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Carbon Monoxide and Water vapor can react to form Carbon Dioxide and Hydrogen. The reaction has a $\Delta H=-41\frac{kJ}{mol}$ , and an equilibrium constant $K= 0.221$ . A 1L canister at 5atm and 25ºC contains equal amounts by volume of Carbon Monoxide and Water. What is the equilibrium mass of Hydrogen gas in the canister?
$CO_{(g)}+H_2O_{(g)}\leftrightarrow CO_{2(g)}+H_{2(g)}$

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Reviewed replacement: in an irreversible first-order disappearance model, [NO₂⁻] starts at 4.00 M and k=42.1 day⁻¹. Find its half-life. This formal model does not claim to describe the original reversible gas-producing reaction.

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Reviewed replacement: A(g)+B(g)⇌2 C(g) in an ideal 5.00 L vessel at 273.15 K has K_c=13.21. Initially there is 1.00 mol each A and B and no C. Calculate equilibrium moles and total pressure, using R=0.082057 L atm mol⁻¹ K⁻¹.

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Reviewed replacement: a specified reaction has ΔH=−481.1 kJ per mole of reaction as written. Independent equilibrium analysis establishes that its forward extent is 0.250 mol. What is the system’s enthalpy change?

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Reviewed replacement: a formal irreversible disappearance law −d[A]/dt=k[A]² has k=4.20 L mol⁻¹ h⁻¹ and [A]₀=0.100 M. How long until [A]=0.0500 M?

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Reviewed replacement: 0.0100 mol Zn reacts with excess dilute nonoxidizing acid by Zn(s)+2 H⁺(aq)→Zn²⁺(aq)+H₂(g). Assuming quantitative reaction, how many moles of hydrogen form?

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Reviewed replacement: an abstract reactant A undergoes irreversible first-order disappearance with k=0.004333 min⁻¹ and [A]₀=0.150 M. Calculate [A] after 10.0 min and 120 min.

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Reviewed replacement: for a stipulated hot-alkali stoichiometric model, 3 Cl₂+6 OH⁻→ClO₃⁻+5 Cl⁻+3 H₂O. How many moles of Cl₂ react when 99.0% of an initial 0.500 mol OH⁻ is consumed? This is a paper stoichiometry exercise.

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Reviewed replacement: in an irreversible first-order disappearance model with k=0.3211 day⁻¹, find the time to consume 90.0% of a reactant.

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Reviewed replacement: a closed ideal gas system contains H₂(g)+Cl₂(g)⇌2 HCl(g), with K_p=4.19 at the specified temperature. Initial partial pressures are p(H₂)=p(Cl₂)=1.00 atm and p(HCl)=0. Find equilibrium partial pressures in the same convention.

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Unfinished source problem slots

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Unfinished source problem slots

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