consider the following equation in chemical equilibrium.\nc₂h₄(g) + h₂(g) ⇌ c₂h₆(g) + 137 kj\nwhat happens…

consider the following equation in chemical equilibrium.\nc₂h₄(g) + h₂(g) ⇌ c₂h₆(g) + 137 kj\nwhat happens to the amount of ethane (c₂h₆) when the temperature of the system is increased?\nthe amount of ethane decreases.\nthe amount of ethane increases initially and then decreases.\nthe amount of ethane increases.\nthe amount of ethane decreases initially and then increases.

consider the following equation in chemical equilibrium.\nc₂h₄(g) + h₂(g) ⇌ c₂h₆(g) + 137 kj\nwhat happens to the amount of ethane (c₂h₆) when the temperature of the system is increased?\nthe amount of ethane decreases.\nthe amount of ethane increases initially and then decreases.\nthe amount of ethane increases.\nthe amount of ethane decreases initially and then increases.

Answer

Brief Explanations:

This is an exothermic reaction (heat is a product as indicated by + 137 kJ). According to Le - Chatelier's principle, when the temperature of an exothermic reaction at equilibrium is increased, the system shifts in the direction that consumes heat, which is the reverse direction. So the amount of the product (ethane, $C_2H_6$) decreases.

Answer:

The amount of ethane decreases.