Answer
The missing values are, respectively (top to bottom):
$$K_C = 617$$
$$[H_2] = 0.343 \space M$$
$$[HI] = 0.338 \space M$$
Work Step by Step
(a)
1. Write the equilibrium constant expression:
- The exponent of each concentration is equal to its balance coefficient.
$$K_C = \frac{[Products]}{[Reactants]} = \frac{[ HI ] ^{ 2 }}{[ H_2 ][ I_2 ]}$$
2. Substitute the values and calculate the constant value:
$$K_C = \frac{( 0.922 )^{ 2 }}{( 0.0355 )( 0.0388 )} = 617$$
(b)
2. Solve for the missing concentration:
$$ [H_2] = \frac{[ HI ]^{ 2 }}{[ I_2 ]\times K_c}$$
3. Evaluate the expression:
$$ [H_2] = \frac{( 0.387 )^{ 2 }}{( 0.0455 )\times(9.6)} $$
$$[H_2] = 0.343 \space M$$
(c)
2. Solve for the missing concentration:
$$ \sqrt[2]{K_c \times [ H_2 ][ I_2 ]}{} = [HI]$$
3. Evaluate the expression:
$$ [HI] = \sqrt[2]{(50.2) \times {( 0.0485 )( 0.0468 )}{}}$$
$$[HI] = 0.338 \space M$$
