Chemistry (4th Edition)

Published by McGraw-Hill Publishing Company

Chapter 15 - Questions and Problems - Page 706: 15.9

Answer

(a) $$K_c = \frac{[ N_2 ][ H_2O ]^{ 2 }}{[ NO ]^{ 2 }[ H_2 ]^{ 2 }}$$ (b) $K_c = 720 = 7.2 \times 10^2$

Work Step by Step

1. Write the equilibrium constant expression: - The exponent of each concentration is equal to its balance coefficient. $$K_c = \frac{[Products]}{[Reactants]} = \frac{[ N_2 ][ H_2O ]^{ 2 }}{[ NO ]^{ 2 }[ H_2 ]^{ 2 }}$$ 2. Substitute the values and calculate the constant value: $$K_c = \frac{( 0.082 )( 4.64 )^{ 2 }}{( 0.31 )^{ 2 }( 0.16 )^{ 2 }} = 720$$

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