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

The reaction will proceed to the left to attain equilibrium.

Step-by-step 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)=(2.50mol* (0.08206atm.L/mol.K)* 673K)/(25.0L) =5.52atm`

`pP_(2)=(1.50mol* (0.08206atm.L/mol.K)* 673K)/(25.0L)=3.31atm`

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

`Qp=(pP_(2)^(2))/(pP_(4)) =(3.31^(2) )/(5.52) =1.98`

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