Question

2 C2H6(9) +7 O2(g) -> 4CO2(g) + 6H2O(g). AH = -1560.7 kJ/mol Which direction with the equilibrium shift if the temperature is decreased?​

Answer 1

If temperature is decreased for an exothermic reaction like 2 C2H6(g) + 7 O2(g) -> 4 CO2(g) + 6 H2O(g), the equilibrium shifts to the left, favoring the formation of reactants.

Step-by-step explanation:

The question pertains to the direction of equilibrium shift when the temperature is decreased for an exothermic reaction represented by 2 C2H6(g) + 7 O2(g) -> 4 CO2(g) + 6 H2O(g) with an enthalpy change ΔH = -1560.7 kJ/mol. According to Le Chatelier's principle, if we decrease the temperature of an exothermic reaction, the equilibrium will shift in the direction that produces heat to counterbalance the imposed change, meaning the reaction will favor the formation of reactants. In this case, the equilibrium will shift to the left, favoring the formation of C2H6 and O2.