Answer
a. $K_c = \frac{[ CO_2 ][ H_2 ]}{[ CO ][ H_2O ]}$
b. $K_c = [CO_2]$
c. $K_c = \frac{[ CH_4 ]^{ 2 }[ Cl_2 ]^{ 3 }}{[ CHCl_3 ]^{ 2 }[ H_2 ]^{ 3 }}$
d. $K_c = \frac{[ HI ]^{ 2 }}{[ H_2 ][ I_2 ]}$
e. $K_c = \frac{[ NO ]^{ 2 }[ Cl_2 ]}{[ NOCl ]^{ 2 }}$
Work Step by Step
Write the equilibrium constant expression:
- The exponent of each concentration is equal to its balance coefficient.
- Pure solids and liquids do not appear in the equation.
a. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ CO_2 ][ H_2 ]}{[ CO ][ H_2O ]}$
b. $K_c = \frac{[Products]}{[Reactants]} = [CO_2]$
c. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ CH_4 ]^{ 2 }[ Cl_2 ]^{ 3 }}{[ CHCl_3 ]^{ 2 }[ H_2 ]^{ 3 }}$
d. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ HI ]^{ 2 }}{[ H_2 ][ I_2 ]}$
e. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ NO ]^{ 2 }[ Cl_2 ]}{[ NOCl ]^{ 2 }}$
