   Chapter 15, Problem 23PS

Chapter
Section
Textbook Problem

Calculate K for the reactionSnO2(s) + 2 CO(g) ⇄ Sn(s) + 2 CO2(g)given the following information: SnO 2 (s) + 2 H 2 (g)  ⇄  Sn(s) + 2 H 2 O(g) K  = 8 .12 H 2 (g) + CO 2 (g)  ⇄  H 2 O(g) + CO(g) K  = 0 .771

Interpretation Introduction

Interpretation: The equilibrium constant of the given reaction has to be calculated.

Concept introduction:

Equilibrium constant: It is the ratio of products to reactants has a constant value when the reaction is in equilibrium at a certain temperature. And it is represented by the letter K.

For a reaction,

aA+bBcC+dD

The equilibrium constant is, K=[C]c[D]d[A]a[B]b, where, a, b, c and d are the stoichiometric coefficients of reactant and product in the reactions.

Explanation

The equilibrium constant of the given reaction is calculated.

Given,

The balanced chemical equation for the first reaction is,

SnO2(s)+2CO(g)Sn(s)+2CO2(g)                     (a)

The equilibrium constant, K1 for the reaction is,

K1=[CO2]2[CO]2

The balanced chemical equation for the second reaction is

SnO2(s)+2H2(g)Sn(s)+2H2O(g)                     (b)

The equilibrium constant, K2 for the reaction is,

K2=[H2O]2[H2]2=8

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