JEE MAIN - Chemistry (2005 - No. 6)
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?
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
Explanation
The reaction given is an exothermic reaction thus accordingly to Lechatalier's principle lowering of temperature, addition of $${F_2}$$ and or $$C{l_2}$$ favour the for ward direction and hence the production of $$Cl{F_3}.$$
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