For the reaction of A and B forming C, A(g)+ B(s)⇌ 2C(g) how will the reaction respond to each of the following changes at equilibrium? Drag the appropriate items to their respective bins.
a) double the concentration of B and halve the concentration of C.
b) double the concentrations of both products and then quadruple the container volume.
c) double the container volume.
d) double the concentrations of both products.
e) add more A.
f) double the concentrations of both products and then double the container volume.

a) forward reaction is favoured producing more of C

b) forward reaction is favoured producing more of C

c) no effect on the reaction rate

d) no effect

e) forward reaction is favoured producing more of C

f) backward reaction will be favoured leading to production of more A and B

Explanation:

The change in equilibrium is explained by le chatelie's principle which states that if some factors of equilibrium of a reaction like concentration, pressure or temperature is altered, the equilibrium position will adjust to cancel the effects of the change.

the millers tale is the answer.

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