The exothermic formation of ClF3 is represented by the equation: Cl2 (g) + 3F2 (g) $\leftrightharpoons$ 2ClF3 (g); $\Delta H$ = -329 kJ Which of the following will increase the quantity of ClF3 in an equilibrium mixture of Cl2, F2 and ClF3?

Question

The exothermic formation of ClF₃ is represented by the equation:
Cl₂ (g) + 3F₂ (g) $\leftrightharpoons$ 2ClF₃ (g); $\Delta H$ = -329 kJ
Which of the following will increase the quantity of ClF₃ in an equilibrium mixture of Cl₂, F₂ and ClF₃?

Increasing the temperature

Removing Cl₂

Increasing the volume of the container

Adding F₂

Solution

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