Question

How would each of the following changes affect this equilibrium? 2 S(s) + 3 O2(g) ⇌ 2 SO3(g); ΔH = −791.4 kJ/mol (a) increasing the temperature Would it shift the reaction toward the reactants? Would it shift the reaction toward the products? Or, does temp not affect equilibrium? (b) increasing [O2] Does increasing O2 shifts the reaction toward the reactants, shift the reaction toward the products, or does the increasing O2 not affect equilibrium? (c) increasing the volume of the container Same question - shifts the reaction toward the reactants? shifts the reaction toward the products? does not affect equilibrium? (d) adding S shifts the reaction toward the reactants? shifts the reaction toward the products? does not affect equilibrium? (e) adding an inert gas to increase the pressure shifts the reaction toward the reactants? shifts the reaction toward the products ? does not affect equilibrium?

Answer 1