Chemistry 9th Edition

Published by Cengage Learning
ISBN 10: 1133611095
ISBN 13: 978-1-13361-109-7

Chapter 13 - Chemical Equilibrium - Exercises - Page 644: 27


K = $1.6\times10^{-7}$

Work Step by Step

According to the law of mass action, a general formula of the form jA + kB ⇌ lC + mD is represented by the following equilibrium expression: K = $\frac{[C]^{l}[D]^{m}}{[A]^{j}[B]^{k}}$ where A, B, C, and D represent the chemical species and j, k, l, and m are their coefficients in the balanced equation. - Work - First, we must calculate the concentrations: $[NO] = 4.5\times10^{3}mol \div 3.0L = 1.5\times10^{3}M$ $[Cl_{2}] = 2.4mol \div 3.0L = 8.0\times10^{-1}M$ $[NOCl] = 1.0mol \div 3.0L = 3.33\times10^{-1}M$ (one extra significant digit carried) K = $\frac{[NO_{2}]^{2}[Cl_{2}]}{[NOCl]^{2}}$ K = $\frac{(1.5\times10^{-3})^{2}(8.0\times10^{-1})}{(3.33\times10^{-1})^{2}}$ K = $1.62\times10^{-7}$ (carried one extra significant digits) K = $1.6\times10^{-7}$
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