Answer
$$K_c = 2.6 \times 10^4$$
$$K_p = 3.2 \times 10^{2} $$
Work Step by Step
1. Since the equation was inverted, the new $K_c$ is equal to the inverse of the original constant value:
$$K'_c = \frac{1}{3.8 \times 10^{-5}} = 2.6 \times 10^4$$
2. Calculate $\Delta n$ (n is the amount of moles of gases):
$$\Delta n = n_{products} - n_{reactants} = 1 - 2 = -1 $$
3. Convert the temperature to Kelvin:
$$T/K = 727 + 273.15 = 1000.15 $$
4. Calculate Kp:
$$K_p = K_c(RT)^{\Delta n} = ( 2.6 \times 10^{4} )(0.0821 \times 1000.15 )^{ -1 }$$
$$K_p = 3.2 \times 10^{2} $$
