/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 26 Consider the equilibrium \(\math... [FREE SOLUTION] | 91影视

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Chapter 15: Problem 26

Consider the equilibrium \(\mathrm{Na}_{2} \mathrm{O}(s)+\mathrm{SO}_{2}(g) \rightleftharpoons\) \(\mathrm{Na}_{2} \mathrm{SO}_{3}(\mathrm{~s}) .\) (a) Write the equilibrium- constant expression for this reaction in terms of partial pressures. (b) Why doesn't the concentration of \(\mathrm{Na}_{2} \mathrm{O}\) appear in the equilibrium-constant expression?

Short Answer

Expert verified
(a) The equilibrium constant expression in terms of partial pressures for the given reaction is: \(K_p = \frac{P_{\mathrm{Na}_{2} \mathrm{SO}_{3}}}{P_{\mathrm{SO}_{2}}}\) (b) The concentration of Na鈧侽 does not appear in the equilibrium-constant expression because it is a solid. The equilibrium constant expression only includes terms for gaseous species and species in the dissolved state, while the concentration of solids does not change during the reaction and does not affect the equilibrium.

Step by step solution

01

(a) Writing the equilibrium constant expression

Recall that the equilibrium constant expression for a reaction relates the concentrations or partial pressures of products and reactants to their stoichiometric coefficients. Since we are asked to express the equilibrium constant in terms of partial pressures, we will use the equilibrium constant K_p. For the given reaction, the K_p expression is: \(K_p = \frac{P_{\mathrm{Na}_{2} \mathrm{SO}_{3}}}{P_{\mathrm{SO}_{2}}}\) Here, \(P_{\mathrm{Na}_{2} \mathrm{SO}_{3}}\) is the partial pressure of Na鈧係O鈧�, and \(P_{\mathrm{SO}_{2}}\) is the partial pressure of SO鈧�. Note that we have not included the Na鈧侽 in the expression. We will explain this in part (b).
02

(b) Explaining the absence of Na鈧侽

The equilibrium constant expression only includes terms for gaseous species and species in the dissolved state. For solids, their concentration does not change during the reaction, and they do not affect the equilibrium. Since Na鈧侽 is in the solid state, its concentration does not appear in the equilibrium constant expression. Instead, its presence is essential to maintain the reaction but does not appear in the equilibrium expression.

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Most popular questions from this chapter

The equilibrium constant for the reaction $$ 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{NOBr}(g) $$ is \(K_{c}=1.3 \times 10^{-2}\) at \(1000 \mathrm{~K} .\) (a) Calculate \(K_{c}\) for \(2 \mathrm{NOBr}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g)\) (b) At this temperature does the equilibrium favor \(\mathrm{NO}\) and \(\mathrm{Br}_{2}\), or does it favor NOBr?

At \(900 \mathrm{~K}\) the following reaction has \(K_{p}=0.345:\) $$ 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) $$ In an equilibrium mixture the partial pressures of \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) are \(0.135 \mathrm{~atm}\) and \(0.455 \mathrm{~atm}\), respectively. What is the equilibrium partial pressure of \(\mathrm{SO}_{3}\) in the mixture?

Suppose that the gas-phase reactions \(\mathrm{A} \longrightarrow \mathrm{B}\) and \(\mathrm{B} \longrightarrow \mathrm{A}\) are both elementary processes with rate con- stants of \(3.8 \times 10^{-2} \mathrm{~s}^{-1}\) and \(3.1 \times 10^{-1} \mathrm{~s}^{-1}\), respectively. (a) What is the value of the equilibrium constant for the equilibrium \(\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g) ?\) (b) Which is greater at equilibrium, the partial pressure of A or the partial pressure of B? Explain.

Silver chloride, \(\mathrm{AgCl}(s)\), is an insoluble strong electrolyte. (a) Write the equation for the dissolution of \(\mathrm{AgCl}(s)\) in \(\mathrm{H}_{2} \mathrm{O}(l)\) (b) Write the expression for \(K_{c}\) for the reaction in part (a). (c) Based on the thermochemical data in Appendix \(\mathrm{C}\) and Le Ch芒telier's principle, predict whether the solubility of \(\mathrm{AgCl}\) in \(\mathrm{H}_{2} \mathrm{O}\) increases or decreases with increasing temperature.

If \(K_{c}=0.042\) for \(\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g)\) at \(500 \mathrm{~K}\), what is the value of \(K_{p}\) for this reaction at this temperature?
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