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Chapter 13: Problem 38

Write expressions for \(K_{\mathrm{p}}\) for the following reactions. a. $2 \mathrm{Fe}(s)+\frac{3}{2} \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{Fe}_{2} \mathrm{O}_{3}(s)$ b. $\mathrm{CO}_{2}(g)+\mathrm{MgO}(s) \rightleftharpoons \mathrm{MgCO}_{3}(s)$ c. $\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)$ d. $4 \mathrm{KO}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 4 \mathrm{KOH}(s)+3 \mathrm{O}_{2}(g)$

Short Answer

Expert verified
a. \(K_{\mathrm{p}}=\frac{1}{[\mathrm{O}_{2}]^{\frac{3}{2}}}\) b. \(K_{\mathrm{p}}=[\mathrm{CO}_{2}]\) c. \(K_{\mathrm{p}}=\frac{[\mathrm{CO}][\mathrm{H}_{2}]}{[\mathrm{H}_{2}\mathrm{O}]}\) d. \(K_{\mathrm{p}}=\frac{[\mathrm{O}_{2}]^3}{[\mathrm{H}_{2}\mathrm{O}]^2}\)

Step by step solution

01

Identify the gaseous species

In this reaction, we have O₂(g) as the only gaseous species involved.
02

Expression for Kp

To write the expression for Kp for this reaction, we have: \[K_{\mathrm{p}}=\frac{1}{[\mathrm{O}_{2}]^{\frac{3}{2}}}\] b. $\mathrm{CO}_{2}(g)+\mathrm{MgO}(s) \rightleftharpoons \mathrm{MgCO}_{3}(s)$
03

Identify the gaseous species

In this reaction, we have CO₂(g) as the only gaseous species involved.
04

Expression for Kp

To write the expression for Kp for this reaction, we have: \[K_{\mathrm{p}}=[\mathrm{CO}_{2}]\] c. $\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)$
05

Identify the gaseous species

In this reaction, we have H₂O(g), CO(g), and H₂(g) as the gaseous species involved.
06

Expression for Kp

To write the expression for Kp for this reaction, we have: \[K_{\mathrm{p}}=\frac{[\mathrm{CO}][\mathrm{H}_{2}]}{[\mathrm{H}_{2}\mathrm{O}]}\] d. $4 \mathrm{KO}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 4 \mathrm{KOH}(s)+3 \mathrm{O}_{2}(g)$
07

Identify the gaseous species

In this reaction, we have H₂O(g) and O₂(g) as the gaseous species involved.
08

Expression for Kp

To write the expression for Kp for this reaction, we have: \[K_{\mathrm{p}}=\frac{[\mathrm{O}_{2}]^3}{[\mathrm{H}_{2}\mathrm{O}]^2}\]

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Most popular questions from this chapter

For the reaction $$\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{HBr}(g)$$ \(K_{\mathrm{p}}=3.5 \times 10^{4}\) at 1495 \(\mathrm{K} .\) What is the value of \(K_{\mathrm{p}}\) for the following reactions at 1495 \(\mathrm{K}\) ? a. $\operatorname{HBr}(g) \rightleftharpoons \frac{1}{2} \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{Br}_{2}(g)$ b. \(2 \mathrm{HBr}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g)\) c. $\frac{1}{2} \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{Br}_{2}(g) \rightleftharpoons \mathrm{HBr}(g)$

Given \(K=3.50\) at \(45^{\circ} \mathrm{C}\) for the reaction $$\mathrm{A}(g)+\mathrm{B}(g) \rightleftharpoons \mathrm{C}(g)$$ and \(K=7.10\) at \(45^{\circ} \mathrm{C}\) for the reaction $$2 \mathrm{A}(g)+\mathrm{D}(g) \rightleftharpoons \mathrm{C}(g)$$ what is the value of \(K\) at the same temperature for the reaction $$\mathrm{C}(g)+\mathrm{D}(g) \rightleftharpoons 2 \mathrm{B}(g)$$ What is the value of \(K_{\mathrm{p}}\) at \(45^{\circ} \mathrm{C}\) for the reaction? Starting with 1.50 atm partial pressures of both \(\mathrm{C}\) and \(\mathrm{D},\) what is the mole fraction of \(\mathrm{B}\) once equilibrium is reached?

A 1.00-L flask was filled with 2.00 moles of gaseous \(\mathrm{SO}_{2}\) and 2.00 moles of gaseous \(\mathrm{NO}_{2}\) and heated. After equilibrium was reached, it was found that 1.30 moles of gaseous NO was present. Assume that the reaction $$ \mathrm{SO}_{2}(g)+\mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g)+\mathrm{NO}(g) $$ occurs under these conditions. Calculate the value of the equilibrium constant, \(K,\) for this reaction.

Predict the shift in the equilibrium position that will occur for each of the following reactions when the volume of the reaction container is increased. a. $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$ b. $\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)$ c. \(\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g)\) d. \(\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\) e. $\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$

For the reaction $$2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ it is determined that, at equilibrium at a particular temperature, the concentrations are as follows: $[\mathrm{NO}(g)]=8.1 \times 10^{-3} \mathrm{M}\( \)\left[\mathrm{H}_{2}(g)\right]=4.1 \times 10^{-5} M,\left[\mathrm{N}_{2}(g)\right]=5.3 \times 10^{-2} M,$ and \(\left[\mathrm{H}_{2} \mathrm{O}(g)\right]-2.9 \times 10^{-3} \mathrm{M} .\) Calculate the value of \(K\) for the reaction at this temperature.
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