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Chapter 15: Problem 110

In the reaction \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}), K=1.0 \times\) \(10^{5}\) at \(25^{\circ} \mathrm{C} .\) Would you expect a greater amount of product or reactant?

Short Answer

Expert verified
There will be a greater amount of product (\(H_{2}O_{2}(aq)\)) at equilibrium.

Step by step solution

01

Understand the reaction

In this reaction, hydrogen peroxide gas, \( H_{2}O_{2}(g) \), is converted into aqueous hydrogen peroxide, \( H_{2}O_{2}(aq) \). This reaction can go both ways, meaning the gas can become aqueous, or the aqueous form can become a gas.
02

Understand the implications of K

The equilibrium constant, K, is a measure of the ratio of concentrations of products to reactants at equilibrium. If K > 1, there are more products than reactants at equilibrium, since the numerator (products) would be larger than the denominator (reactants). If K < 1, there are more reactants than products.
03

Apply K to this reaction

In this case, K=1.0x\(10^{5}\), which is much larger than 1. Therefore, at equilibrium, there would be more product (\(H_{2}O_{2}(aq)\)) than reactant (\(H_{2}O_{2}(g)\)).

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Most popular questions from this chapter

Can a mixture of \(2.2 \mathrm{mol} \mathrm{O}_{2}, 3.6 \mathrm{mol} \mathrm{SO}_{2},\) and \(1.8 \mathrm{mol}\) \(\mathrm{SO}_{3}\) be maintained indefinitely in a \(7.2 \mathrm{L}\) flask at a temperature at which \(K_{\mathrm{c}}=100\) in this reaction? Explain. $$ 2 \mathrm{SO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{g}) $$

For the reaction $$ \mathrm{A}(\mathrm{s}) \rightleftharpoons \mathrm{B}(\mathrm{s})+2 \mathrm{C}(\mathrm{g})+\frac{1}{2} \mathrm{D}(\mathrm{g}) \quad \Delta H^{\circ}=0 $$ (a) Will \(K_{p}\) increase, decrease, or remain constant with temperature? Explain. (b) If a constant-volume mixture at equilibrium at 298 K is heated to 400 K and equilibrium re-established, will the number of moles of \(\mathrm{D}(\mathrm{g})\) increase, decrease, or remain constant? Explain.

Explain the important distinctions between each pair of terms: (a) reaction that goes to completion and reversible reaction; (b) \(K_{\mathrm{c}}\) and \(K_{\mathrm{p}} ;\) (c) reaction quotient (Q) and equilibrium constant expression ( \(K\) ); (d) homogeneous and heterogeneous reaction.

Write equilibrium constant expressions, \(K_{\mathrm{c}},\) for the reactions (a) \(2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{g})\) (b) \(\mathrm{Zn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) (c) \(\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{CO}_{3}^{2-}(\mathrm{aq}) \rightleftharpoons\) \(\mathrm{MgCO}_{3}(\mathrm{s})+2 \mathrm{OH}^{-}(\mathrm{aq})\)

A mixture of \(1.00 \mathrm{mol} \mathrm{NaHCO}_{3}(\mathrm{s})\) and \(1.00 \mathrm{mol}\) \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{s})\) is introduced into a \(2.50 \mathrm{L}\) flask in which the partial pressure of \(\mathrm{CO}_{2}\) is 2.10 atm and that of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) is \(715 \mathrm{mmHg} .\) When equilibrium is established at \(100^{\circ} \mathrm{C},\) will the partial pressures of \(\mathrm{CO}_{2}(\mathrm{g})\) and \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) be greater or less than their initial partial pressures? Explain. $$\begin{array}{r} 2 \mathrm{NaHCO}_{3}(\mathrm{s}) \rightleftharpoons \mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \\ K_{\mathrm{p}}=0.23 \mathrm{at} 100^{\circ} \mathrm{C} \end{array}$$
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