Answer
a. $K_c = \frac{[ H_{2}O ]^{ 2 }[ O_{2} ]^{ }}{[ H_{2}O_{2} ]^{ 2 }}$
b. $K_c = \frac{[ SO_{2} ]^{ 2 }}{[ O_{2} ]^{ 3 }}$
c. $K_c = \frac{1}{[ NH_{3} ][ HCl ]}$
d. $K_c = \frac{[ NO_{2} ]^{ 2 }}{[ N_{2}O_{4} ]}$
e. $K_c = \frac{[ HCl ]^{ 4 }[ O_{2} ]^{ }}{[ Cl_{2} ]^{ 2 }[ H_{2}O ]^{ 2 }}$
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. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ H_{2}O ]^{ 2 }[ O_{2} ]^{ }}{[ H_{2}O_{2} ]^{ 2 }}$
b. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ SO_{2} ]^{ 2 }}{[ O_{2} ]^{ 3 }}$
c. $K_c = \frac{[Products]}{[Reactants]} = \frac{1}{[ NH_{3} ][ HCl ]}$
d. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ NO_{2} ]^{ 2 }}{[ N_{2}O_{4} ]}$
e. $K_c = \frac{[Products]}{[Reactants]} = \frac{[ HCl ]^{ 4 }[ O_{2} ]^{ }}{[ Cl_{2} ]^{ 2 }[ H_{2}O ]^{ 2 }}$
