Home
Class 12
CHEMISTRY
Given the equilibrium system NH(4)Cl(s...

Given the equilibrium system
`NH_(4)Cl(s)hArr NH_(4)^(+)(aq)+Cl^(-)(aq) (DeltaH=+"3.5 kcal/mol").`
What change will shift the equilibrium to the right?

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.

Text Solution

AI Generated Solution

The correct Answer is:
To determine what change will shift the equilibrium of the reaction \[ \text{NH}_4\text{Cl}(s) \rightleftharpoons \text{NH}_4^+(aq) + \text{Cl}^-(aq) \quad (\Delta H = +3.5 \text{ kcal/mol}) \] to the right (towards the products), we need to consider the principles of Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. ### Step-by-Step Solution: 1. **Identify the Nature of the Reaction**: - The reaction is endothermic, as indicated by the positive ΔH value (+3.5 kcal/mol). This means that heat is absorbed when the reaction proceeds in the forward direction (producing NH4+ and Cl-). 2. **Evaluate Temperature Changes**: - For an endothermic reaction, increasing the temperature will shift the equilibrium to the right (towards the products) because the system will absorb the added heat. - Conversely, decreasing the temperature will shift the equilibrium to the left (towards the reactants). 3. **Consider Concentration Changes**: - Adding more products (NH4+ or Cl-) will shift the equilibrium to the left to reduce the concentration of the added products. - Therefore, adding NH4NO3 (which provides NH4+) or NaCl (which provides Cl-) will shift the equilibrium to the left. 4. **Conclusion**: - The only change that will shift the equilibrium to the right is increasing the temperature. ### Final Answer: Increasing the temperature will shift the equilibrium to the right.
Promotional Banner

Similar Questions

Explore conceptually related problems

The equilibrium pressure of NH_(4)CN(s) hArr NH_(3)(g)+HCN(g) is 2.98 atm. Calculate K_(p)

For the equilibrium NH_2CONH_4(s) hArr 2NH_3(g) +CO_2(g) P_(CO_2)= 1 atm at 100^@C . What will be the equilibrium constant at 100^@C in atm.

NH_(4)CI(s) + aq rarr NH_(4)^(+)(aq) + CI^(-1)(aq) DeltaH=+15.1 KJ mol^(-1) NH_(4)CI(s) dissolves in water according to above equation

On decomposition of NH_(4)HS , the following equilibrium is estabilished: NH_(4) HS(s)hArrNH_(3)(g) + H_(2)S(g) If the total pressure is P atm, then the equilibrium constant K_(p) is equal to

In the equilibrium NH_(4) HS_(s) hArr NH_(3(g)) + H_(2) S_((g)) . the forward reaction can be favoured by

For the process NH_(3)(g) +HCI(g) rarr NH_(4)Cl(s)

Consider the chemical reaction: underset(("Green solution"))(Ni^(2+)(aq))+6NH_(3)(aq) hArr underset(("Blue solution"))([Ni(NH_(3))_(6)]^(2+)) (aq) When H^(o+)(aq) is added, the colour green is favoured. Use one or more of the following interpretations to answer the questions: i. Some unreacted Ni^(2+)(aq) is present in the solution at equilibrium ii. Some unreacted NH_(3)(aq) is present in the solution at equilibrium iii. The colour change indicates new equilibrium conditions with reduced [Ni(NH_(3))_(6)]^(2+)(aq) iv. The colour change indicates new equilibrium conditions with increased [Ni(NH_(3))_(6)]^(2+)(aq) . The deepening of blue colour on addition of more NH_(3)(aq) supports interpretation(s).

Decomposition of ammonium chloride is an endothermic reaction. The equilibrium may be represented as: NH_(4)Cl(s) hArr NH_(3)(g)+HCl(g) A 6.250 g sample of NH_(4)Cl os placed in an evaculated 4.0 L container at 27^(@)C . After equilibrium the total pressure inside the container is 0.820 bar and some solid remains in the container. Answer the followings The amount of solid NH_(4)Cl left behind in the container at equilibrium is

Consider the chemical reaction: underset(("Green solution"))(Ni^(2+)(aq))+6NH_(3)(aq) hArr underset(("Blue solution"))([Ni(NH_(3))_(6)]^(2+)) (aq) When H^(o+)(aq) is added, the colour green is favoured. Use one or more of the following interpretations to answer the questions: i. Some unreacted Ni^(2+)(aq) is present in the solution at equilibrium ii. Some unreacted NH_(3)(aq) is present in the solution at equilibrium iii. The colour change indicates new equilibrium conditions with reduced [Ni(NH_(3))_(6)]^(2+)(aq) iv. The colour change indicates new equilibrium conditions with increased [Ni(NH_(3))_(6)]^(2+)(aq) . The deepening of blue colour on dissolving more Ni(NO_(3))_(2) supports interpretation (s).

For the following equilibrium NH_(3)+H_(2)O hArr NH_(4)^(+)+OH^(-) calculate the equilibrium constant, if for the equilibrium, NH_(4)^(+)+H_(2)OhArr NH_(4)OH+H^(+) the equilibrium constant is 5.5xx10^(-10)