Which of the following are true statements about equilibrium systems? For the fo

Question

Which of the following are true statements about equilibrium systems? For the following reaction at equilibrium:

H2(g) + F2(g) ? 2HF(g) removing H2 will increase the amount of F2 present once equilibrium is reestablished.

For the following reaction at equilibrium: CaCO3(s) ? CaO(s) + CO2(g) increasing the total pressure by adding Ar(g) will shift the equilibrium to the left.

For the following reaction at equilibrium: 2 H2(g) + O2(g) ? 2 H2O(g) the equilibrium will shift to the right if the volume is halved.

For the following reaction at equilibrium: CaCO3(s) ? CaO(s) + CO2(g) adding more CaCO3 will shift the equilibrium to the right.

Increasing the temperature of an exothermic reaction shifts the equilibrium position to the left.

Explanation / Answer

First statement is true because removing H2 will shift the reaction towards the left.

Second statement is false because increasing the total pressure by adding inert gas at constant volume has no effect on equilibrium.

Third statement is true because decreasing volume shifts the reaction towards the side containing fewer moles of gas.

Fourth statement is right because increasing reactant conc shifts reaction towards right.

Fifth statement is true because in exothermic reaction heat is on the product side, so when temperature is increased, reaction shifts towards left.

Hope this helps !

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