Consider the following system at equilibrium: N2(g) + 3H2(g) 2NH3(g); delta H de
ID: 771485 • Letter: C
Question
Consider the following system at equilibrium: N2(g) + 3H2(g) 2NH3(g); delta H degree = -92.94 kJ Which of the following changes will shift the equilibrium to the right? increasing the temperature decreasing the temperature increasing the volume decreasing the volume removing some NH3 adding some NH3 removing some N2 adding some N2 II, III, V, VIII I, VI, VII I, III, V, VII I, IV, VI, VII II, IV, V, VIIIExplanation / Answer
It is an exothermic rxn, so dectease in temp. favours forward rxn (II) , Decrease in vol. => increase in pressure, So system will move to the direction on which pressure is less therefore forward (IV), Removing NH3 will move the reaction forward (V), Adding N2 will move rxn forward (VIII)...Hence option E