#### Answer

d)
$[ A ] = 0.70 \space M$
$[ B ] = 0.70 \space M$
$[ C ] = 0.092 \space M$

#### Work Step by Step

1. Write the equilibrium constant expression:
- The exponent of each concentration is equal to its balance coefficient.
$$K_c = \frac{[Products]}{[Reactants]} = \frac{[ C ]^{ 2 }}{[ A ][ B ]}$$
2. At equilibrium, these are the concentrations of each compound:
$[ A ] = 0.750 \space M - x$
$[ B ] = 0.750 \space M - x$
$[ C ] = 2x$
$$1.7 \times 10^{-2} = \frac{(2x)^2}{(0.750 - x)(0.750 - x)}$$
Solving that equation:
$x = 0.046$
3.
$[ A ] = 0.750 - 0.046 = 0.70 \space M$
$[ B ] = 0.750 \space M - 0.046 = 0.70 \space M$
$[ C ] = 2(0.046) = 0.092 \space M$