Chemistry: Atoms First (2nd Edition)

Published by Cengage Learning
ISBN 10: 1305079248
ISBN 13: 978-1-30507-924-3

Chapter 12 - Exercises - Page 524c: 28

Answer

$$K_C = 4.0 \times 10^{8}$$

Work Step by Step

- Calculate all the concentrations: $$[N_2] = ( 2.80 x 10^{-4} )/(2.00) = 1.40 x 10^{-4} M$$ $$[O_2] = ( 2.50 x 10^{-5} )/(2.00) = 1.25 x 10^{-5} M$$ $$[N_2O] = ( 2.00 x 10^{-2} )/(2.00) = 1.00 x 10^{-2} M$$ - The exponent of each concentration is equal to its balance coefficient. $$K_C = \frac{[Products]}{[Reactants]} = \frac{[ N_2O ] ^{ 2 }}{[ N_2 ] ^{ 2 }[ O_2 ]}$$ 2. Substitute the values and calculate the constant value: $$K_C = \frac{( 1.00 \times 10^{-2} )^{ 2 }}{( 1.40 \times 10^{-4} )^{ 2 }( 1.25 \times 10^{-5} )} = 4.1 \times 10^{8}$$
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