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Chapter 13: Problem 25

Write the equilibrium expression (K) for each of the following gas-phase reactions. a. \(N_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)\) b. \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)\) c. $\operatorname{SiH}_{4}(g)+2 \mathrm{Cl}_{2}(g) \rightleftharpoons \operatorname{SiCl}_{4}(g)+2 \mathrm{H}_{2}(g)$ d. $2 \mathrm{PBr}_{3}(g)+3 \mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{PCl}_{3}(g)+3 \mathrm{Br}_{2}(g)$

Short Answer

Expert verified
a. \(K = \frac{[NO]^2}{[N_2][O_2]}\) b. \(K = \frac{[NO_2]^2}{[N_2O_4]}\) c. \(K = \frac{[SiCl_4][H_2]^2}{[SiH_4][Cl_2]^2}\) d. \(K = \frac{[PCl_3]^2[Br_2]^3}{[PBr_3]^2[Cl_2]^3}\)

Step by step solution

01

Identify reactants and products

In this reaction, N₂(g) and O₂(g) are the reactants and 2NO(g) is the product.
02

Write the equilibrium expression

The equilibrium constant expression (K) for the reaction is given by: \(K = \frac{[NO]^2}{[N_2][O_2]}\) b. N₂O₄(g) ⇌ 2NO₂(g)
03

Identify reactants and products

In this reaction, N₂O₄(g) is the reactant, and 2NO₂(g) is the product.
04

Write the equilibrium expression

The equilibrium constant expression (K) for the reaction is given by: \(K = \frac{[NO_2]^2}{[N_2O_4]}\) c. SiH₄(g) + 2Cl₂(g) ⇌ SiCl₄(g) + 2H₂(g)
05

Identify reactants and products

In this reaction, SiH₄(g) and 2Cl₂(g) are the reactants, and SiCl₄(g) and 2H₂(g) are the products.
06

Write the equilibrium expression

The equilibrium constant expression (K) for the reaction is given by: \(K = \frac{[SiCl_4][H_2]^2}{[SiH_4][Cl_2]^2}\) d. 2PBr₃(g) + 3Cl₂(g) ⇌ 2PCl₃(g) + 3Br₂(g)
07

Identify reactants and products

In this reaction, 2PBr₃(g) and 3Cl₂(g) are the reactants, and 2PCl₃(g) and 3Br₂(g) are the products.
08

Write the equilibrium expression

The equilibrium constant expression (K) for the reaction is given by: \(K = \frac{[PCl_3]^2[Br_2]^3}{[PBr_3]^2[Cl_2]^3}\)

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Most popular questions from this chapter

At a particular temperature, \(K=1.00 \times 10^{2}\) for the reaction $$\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \leftrightharpoons 2 \mathrm{HI}(g)$$ In an experiment, 1.00 mole of \(\mathrm{H}_{2}, 1.00\) mole of \(\mathrm{I}_{2},\) and 1.00 mole of \(\mathrm{HI}\) are introduced into a \(1.00-\mathrm{L}\) container. Calculate the concentrations of all species when equilibrium is reached.

At a particular temperature, \(K=3.75\) for the reaction $$\mathrm{SO}_{2}(g)+\mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g)+\mathrm{NO}(g)$$ If all four gases had initial concentrations of \(0.800 M,\) calculate the equilibrium concentrations of the gases.

In a given experiment, 5.2 moles of pure NOCl were placed in an otherwise empty \(2.0-\mathrm{L}\) container. Equilibrium was established by the following reaction: $$2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \quad K=1.6 \times 10^{-5}$$ a. Using numerical values for the concentrations in the Initial row and expressions containing the variable \(x\) in both the Change and Equilibrium rows, complete the following table summarizing what happens as this reaction reaches equilibrium. Let \(x=\) the concentration of \(\mathrm{Cl}_{2}\) that is present at equilibrium. b. Calculate the equilibrium concentrations for all species.

At \(35^{\circ} \mathrm{C}, K=1.6 \times 10^{-5}\) for the reaction $$2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g)$$ Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure \(\mathrm{NOCl}\) in a 2.0 \(\mathrm{L}\) flask b. 1.0 mole of NOCl and 1.0 mole of NO in a 1.0 - flask c. 2.0 moles of \(\mathrm{NOCl}\) and 1.0 mole of \(\mathrm{Cl}_{2}\) in a \(1.0-\mathrm{L}\) flask

For the following endothermic reaction at equilibrium: $$2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g)$$ which of the following changes will increase the value of \(K ?\) a. increasing the temperature b. decreasing the temperature c. removing \(\mathrm{SO}_{3}(g)\) (constant \(T )\) d. decreasing the volume (constant \(T )\) e. adding \(\operatorname{Ne}(g)(\text { constant } T)\) f. adding \(\mathrm{SO}_{2}(g)(\text { constant } T)\) g. adding a catalyst (constant T)
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