Question

At equilibrum at a temperature of 57 °C inside a sealed fixed-volume chamber, there was found to be 0.090 atm of gas A present, 0.290 atm of gas B present and 0.310 atm of gas D present. If more of gas D is pumped into the chamber at constant temperature, such that the new pressure of gas D is 0.100 atm higher than it was before, what is the ΔG of the reaction below now? Assume the extra D gas was pumped in so quickly that during the pumping no amount of reaction occured during the pumping process. Which way will the reaction shift to regain equilibrium after the pumping process is complete?

A(g) + 3B(g) -----> 2D(g)

reaction will shift left or right and why?

Answer 1