Question

Consider the following endothermic reaction in chemical equilibrium: ?A(g) + B (g) ⇋ C(g) + D(s) How many of the following changes will cause the reaction to shift to the left (in the direction of reactants) to re-establish equilibrium?(a) adding some A(g)(b) removing some D(s)(c) increasing the volume of container(d) heating the reaction

Answer 1

There is none of the options that can cause the reaction to shift to the left.

Step-by-step explanation:

If the reaction equation is correct as this A(g) + B (g) ⇋ C(g) + D(s)

• Adding some A would mean increase in concentration of reactant which generally shift the equilibrium to right.

• Removing some D would mean decreasing the concentration of the product which generally shift the reaction to the right.
• increasing the volume would not bring any change to the reaction since there are equal number of moles of gaseous reactant and product.
• heating the reaction that is increasing the temperature would favor forward reaction since the reaction is endothermic which absorbs heat energy

Base on these points, there is none of the options that can cause the reaction to shift to the left.