When NaNO3 is heated in a closed vessel, oxygen is... more liberated and NaNO2 is left behind. At equilibrium.a)Addition of NaNO2 favours reverse reaction.b)Addition of NaNO3 favours forward reaction.c)Increasing temperature favours forward reaction.d)Increasing pressure favours reverse reaction.Correct answer is option 'C,D'. Can you explain this answer?

Question

Answer

I think correct answer must be option 4 bcoz NaNO2 and NaNO3 are in solid state and ng = +ve
increase in pressure favours reverse reaction bcoz reactant side has no gaseous molecules.

Answer

1.increase in concentration of reactant and decrease in concentration of product will shift reaction in forward direction and vice versa
2.exothermic, low temperature forward. Endothermic high temperature forward
3.Endothermic low pressure forward. Exothermic high pressure forward

in this question this is example of Endothermic reaction. that's why C option is correct
I hope I explained.

Answer

Answer:

When NaNO3 is heated in a closed vessel, it decomposes to produce oxygen gas (O2) and sodium nitrite (NaNO2). The reaction can be represented as:

2NaNO3(s) → 2NaNO2(s) + O2(g)

At equilibrium, the forward and reverse reactions are occurring at the same rate. In this case, the equilibrium can be shifted by manipulating the concentration of the reactants and products, as well as the temperature and pressure.

Effect of Addition of NaNO2:
- Addition of NaNO2 would increase the concentration of the product, which would cause the equilibrium to shift in the reverse direction to decrease the concentration of NaNO2. Therefore, option a) is incorrect.

Effect of Addition of NaNO3:
- Addition of NaNO3 would increase the concentration of the reactant, which would cause the equilibrium to shift in the forward direction to decrease the concentration of NaNO3. Therefore, option b) is correct.

Effect of Increasing Temperature:
- According to Le Chatelier's principle, increasing the temperature favors the endothermic reaction. In this case, the forward reaction is endothermic because heat is required to break the bonds in NaNO3. Therefore, increasing the temperature would favor the forward reaction and shift the equilibrium to the right, increasing the production of NaNO2. Hence, option c) is correct.

Effect of Increasing Pressure:
- The reaction does not involve any gases in the reactants or products, so an increase in pressure would not have any significant effect on the equilibrium position. Therefore, option d) is incorrect.

In conclusion, the correct options are c) Increasing temperature favors the forward reaction and d) Increasing pressure does not have any significant effect on the equilibrium position.

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