The following equilibrium in a saturated solution of `NH_4Cl`.
`NH_(4)Cl(s) rarr NH_(4)^(+)(aq) + Cl^(-)(aq) " "DeltaH_(25^@C) = 3.5 Kcal mol(-1)`
A change that will shift the equilibrium to the right is :

Options

A. Decreasing the temperature
B. Increasing the temperature
C. Dissolving NaCl crystals in the equilibrium mixture
D. Dissolving `NH_(4)NO_(3)` crystals in the equilibrium mixture

Answer

B

Explanation

`NH_(4)Cl(s) rarr NH_(4)^(+)(aq) + Cl^(-)(aq), DeltaH = +ve` Increasing temperature will shift the reaction to the right