Question

8. The following exothermic reaction is allowed to reach equilibrium: 2 H2(g) + O2(g) =2H20 (g) a. What happens to the reaction when temperature is decreased? b. What happens to the reaction when temperature is increased? c. What happens to the reaction when H, (g) is added? d. What happens to the reaction when 0; (g) is removed? e. What happens to the reaction when H:0 (g) is removed? f. What happens to the reaction when H,0 (g) is added?

Answer 1

Ans:

As we know for exothermic reaction heat will produce , for exothermic reaction if we increase temperature reaction shifts towards left side which means products will convert to reactant.

While decreasing temperature reaction shifts towards right side which means reactants are converting into products.

From the given reaction

This is exothermic reaction

2H29) +029) = 21,01)

a. If we decrease temperature reaction shifts right side which means reactants are converted into products, which means formation of water

b.If we increase temperature reaction shifts left side which means H2O Will decompose as H2 and O2

c. By increasing reactant concentration reaction shifts towards right side me and product side so water will form by increasing H2 concentration.

d. If we decrease concentration of reactant reaction shifts towards left sidemeans products converted into reactant.

If we remove O2 whcoh means reactants side O2 concentration decrease so reaction shifts from right to left so water will decompose.

e. If H2O removed product concentration decreses so reaction proceed towrds right side so product will form, water will form.

F. If we added water product concentration increses so reaction shifts left side so decomposition of H2O will takes place.

These all conditions happens only as per Lechatleir principle.

Thanking