I wanna check my answers ! The following exothermic reaction is at equilibrium i

Question

I wanna check my answers !

The following exothermic reaction is at equilibrium in a closed container:
2N2O(g) <--> 2N2(g) + O2(g)

#1-5 What will be the effect on the equilibrium position with each of the following disturbances: shift left, shift right, or no effect?
1. The addition of a dinitrogen monoxide gas to the reaction container at constant volume
2. The addition of oxygen gas to the reaction container at constant volume
3. An increase in temperature
4. A decrease in the volume of the reaction container
5. Adding argon gas to the reaction container at constant volume

#6-10 What will be the effect on the equilibrium concentration of N2(g) with each of the following disturbances: increases, decreases, or no effect?
6. The addition of dinitrogen monoxide gas to the reaction container
7. The addition of oxygen gas to the reaction container at constant volume
8. The addition of nitrogen gas to the reaction container at constant volume
9. An increase in temperature
10. The addition of a catalyst to the reaction container

1. R 2. L 3. L 4. L 5. Ne

6. I 7. D 8. I 9. D 10. Ne

Please explain why 8 is increase! thanks

Explanation / Answer

1.(R): When we add reactant(N2O,g) to a chemical reaction in equilibrium, the reaction shifts towards right and more and more products are formed.

2.(L): When we add product(O2,g) to a chemical reaction in equilibrium, the reaction shifts towards left and more and more reactants are formed.

3.(L) Since this is an exothermic reaction, decrease in temperature favors forward reaction (product) and increase in temperature favors backward reaction(reactant). Hence the reactant shifts towards left.

4.(L): As the volume decreases, the pressure inside the container increases. According to Lechatelier's principle, when pressure increases the reaction shift in a direction where number of gaseous moles decreases.

Here the number of gaseous moles decreases from product(3 mol) to reactant(2 mol). Hence the reaction will shift towards reactant(left).

5.(Ne): Addition of inert gas like Ar has no effect on equilibrium.

Hence 1 - 5 are all correct

6.(I):Since N2(g) is a product, addition of a reactant (N2O,g) will shift the reaction towards product. Hence the equilibrium concentration will increase(I).

7.(D): Since N2(g) is a product, addition of another product (O2,g) will shift the reaction towards reactant. Hence the equilibrium concentration will decrease(D).

8.(I): Since N2(g) is a product, addition of N2(g) will shift the reaction towards reactant in order ot keep the equilibrium cnstant same. Hence the concentration of reactant increase to some extent and the concentration of products (N2 and O2) will some extent.

However the decrease in the amount of N2 is less than the amount of N2(g) added, because some of the decrease in the amount of N2 is compensated by increase in the concentration of N2O. Hence the over all equilibrium concentration of N2(g) will increase.

9.(D): Increase in temperature will favor reactant. Hence concentration of N2(g) will decrease.

10.(Ne): Addition of catalyst has no effect on equilibrium concentration.

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