Home
Class 12
CHEMISTRY
The exothermic formation of ClF(3) is re...

The exothermic formation of `ClF_(3)` is represented by thr equation:
`Cl_(2)(g)+3F_(2)(g) hArr 2ClF_(3)(g), DeltaH=-329 kJ`
Which of the following will increase the quantity of `ClF_(3)` in an equilibrium mixture of `Cl_(2), F_(2)`, and `ClF_(3)`?

A

Adding `F_(2)`

B

Increasing the volume of the container

C

Removing `Cl_(2)`

D

Increasing the temperature

Text Solution

Verified by Experts

The correct Answer is:
A
On adding reactant at equilibrium, rate of forward reaction increases.
Promotional Banner

Similar Questions

Explore conceptually related problems

The exothermic formation of C1F_(3) is represented by the equation C1_(2(g)) + 3F_(2(g))hArr2C1F_(3(g)) , Delta H = - 329 kJ Which of the following will increase the quantity of C1F_(3) in an equilibrium mixture of C1_(2) , F_(2) and C1F_(3)

Formation of ClF_(3) from Cl_(2)and F_(2) is an exothermic process . The equilibrium system can be represented as Cl_(2(g))+3F_(2(g))rArr2ClF_(3(g)),DeltaH=-329kJ Which of the following will increase quantity of ClF_(3) in the equilibrium mixture ?

For the reaction : Cl_92)(g)+3F_(2)(g)hArr2ClF_(3)(g),DeltaH=-329 kJ, dissociation of ClF_(3)(g) will be favourate by :

For the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g),DeltaH=-93.6 kJ mol^(-1) . The concentration of H_(2) at equilibrium will increase if