Some of the reactants or the products are in the gaseous phase.
Answer:
Kc = [CH₄] / [H₂]²
Kp = [CH₄] / [H₂]² * (0.082*T)^-1
Explanation:
Equilibrium constant, Kc, is defined as the ratio of the concentrations of the products over the reactants. Also, each concentration of product of reactant is powered to its coefficient.
<em>Pure solids and liquids are not taken into account in an equilibrium</em>
Thus, for the reaction:
C(s)+ 2H₂(g) ⇌ CH₄(g)
Equilibrium constant is:
<h3>Kc = [CH₄] / [H₂]²</h3>
Now, using the formula:
Kp = Kc* (RT)^Δn
<em>Where R is gas constant (0.082atmL/molK), T is the temperature of the reaction and Δn is difference in coefficients of gas products - coefficients of gas reactants (1 - 2= -1)</em>
Replacing:
<h3>Kp = [CH₄] / [H₂]² * (0.082*T)^-1</h3>
<em />
37.8 grams of CS2 equals to 37.8/76=0.5 mole. So the products have 0.5 mole CO2 which is 11.2 liters at STP. So according to the gas law, the volume at given condition is 12.4 liters. So the answer should be 12.2 liters.
