Question

Given that Kp [NOTE: Kp!!!!] = 1.39 at 400 ºC for the reaction, P4(g) <=> 2 P2(g), which answer best describes the reaction when 2.50 mol of P4(g) and 1.50 mol of P2(g) are mixed in a 25.0 L, closed container at 400 ºC? [REMEMBER: it’s Kp]

Answer 1

Answer:

The reaction will proceed to the left to attain equilibrium.

Explanation:

The question is missing but I guess it must be about how the reaction will proceed to attain equilibrium.

First, we have to calculate the partial pressures using the ideal gas equation.

$pP_{4}=\frac{2.50mol\times (0.08206atm.L/mol.K)\times 673K}{25.0L} =5.52atm$

$pP_{2}=\frac{1.50mol\times (0.08206atm.L/mol.K)\times 673K}{25.0L}=3.31atm$

Now, we have to calculate the reaction quotient (Qp).

$Qp=\frac{pP_{2}^{2}}{pP_{4}} =\frac{3.31^{2} }{5.52} =1.98$

Since Qp > Kp, the reaction will proceed to the left to attain equilibrium.