The following reaction has attained equilibrium in a fixed volume container: CO

Question

The following reaction has attained equilibrium in a fixed volume container: CO (g) + H2O (g) CO2 (g) + H2 (g) H-411 kJ Which of the following is CORRECT if the temperature of the system is increased Both the rates of forward and backward reaction increase The pressure of the system remains unchanged The equilibrium constant of the reaction remains unchanged The respective yields of CO2(g) and H2 (g) increase to the same extent There is no change in the amount of compounds because there are equal number of molecules on both sides of equation Last saved at 13:46:13 Finish attem gress Previous page

Explanation / Answer

Option B is the correct answer

In the given equation, there are equal number of moles of reactants and products so the pressure has no effect on equilibrium.

The given equation is exothermic, by increasing the temperature

Rate of reverse reaction > rate of forward reaction

Equilibrium constant decreases

The respective yields of CO and H2 decreases the same extent

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