Consider the following reaction: 2 N2O2 (g) + N2O4 (g) --> 2 N2O3 (g) + 2 NO (g)

Question

Consider the following reaction:
2 N2O2 (g) + N2O4 (g) --> 2 N2O3 (g) + 2 NO (g), withHº = - 32 kJ/mol. Predict the effect of:
(1). removing NO (g) from the equilibrium mixture,
(2). raising the temperature of the equilibrium mixture,
(3). decreasing the volume of the container filled with theequilibrium mixture.


a) (1) shifts right, (2) shifts left, (3) shifts right.
b) (1) shifts right, (2) shifts right, (3) shifts left.
c) (1) shifts left, (2) shifts left, (3) shifts right.
d) (1) shifts right, (2) shifts right, (3) shifts right.
e) (1) shifts left, (2) shifts right, (3) shifts right.
f) (1) shifts left, (2) shifts right, (3) shifts left.
g) (1) shifts right, (2) shifts left, (3) shifts left.
h) (1) shifts left, (2) shifts left, (3) shifts left.

Explanation / Answer

                         2 N2O2 (g) + N2O4 (g) --> 2 N2O3 (g) + 2 NO (g) 1)    removing NO from the mixture As concentration of products decreases, reaction shifts to theright. 2) Since this is an exothermic reaction, raising the temperature,shifts the reaction equilibrium to the left or the reversereaction. 3) Decreasing the volume of the container. Moles of products is more than moles of reactents. So reducing the volume will shift the reaction towardsreactent side i.e left. So answer is : g

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