You know that the equilibrium constant,
To find out, you need to determine the reaction quotient,
In other words, the reaction quotient tells you what reaction is favored at these specific partial pressures in order for the equilibrium to be established.
The equilibrium reaction looks like this
#"CH"_text(4(g]) + "Cl"_text(2(g]) rightleftharpoons "CH"_3"Cl"_text((g]) + "HCl"_text((g])#
By definition, the equilibrium constant is equal to
#K_p = ((P_(HCl)) * (P_(CH_3Cl)))/((P_(CH_4)) * (P_(Cl_2)))#
The expression for
The reaction quotient, on the other hand, uses the partial pressures of the gases at a specific moment
#Q_p = ((P_(HCl))_i * (P_(CH_3Cl))_i)/( (P_text(CH_4))_i * (P_(Cl_2))_i)#
Plug in you values and solve for
#Q_p = (( 0.47color(red)(cancel(color(black)("atm")))) * (0.24color(red)(cancel(color(black)("atm")))))/( (0.13color(red)(cancel(color(black)("atm")))) * (0.035color(red)(cancel(color(black)("atm"))))) = 24.8#
This tells you that the reaction is not at equilibrium.
It's clear that
To reach equilibrium, the forward reaction will be favored, meaning that the equilibrium will shift to the right.
If this is the case, then