2SO2(g) + O2(g) ↔ 2SO3(g)
ΔH = -189 kJ mol-1
The equilibrium constant for the reaction above is increased by?
C(s) + H2O(g) → H2(g) + CO2(g)
ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is?
Two equal bulbs, one containing ammonia and the other nitrogen are opened mouth - to - mouth to each other at room temperature. The entropy in the mixture of gases is likely to?
A catalyst increase the rate of a chemical reaction by providing a path that?
CuO(s) + H\(_2\)(g) ↔ Cu(s) + H\(_2\)O(g)
What is the effect of increasing the pressure on the equilibrium reaction above?
