Question

Q.1 A certain gaseous reaction, carried out in an insulated sealed container results in an increase in temperature from 200 K to 400 K, with the pressure remaining constant. The correct equation that describes the reaction is: 1. 2XY (g) + Y2 (g) → 2XY2 (g)
2. 2XY2 (g) → X₂ (g)+ 2Y2 (g).
3. X(g) + Y2 (g) → XY2 (g)
4 X2 (g) + Y2 (g) → 2XY (g)​

Answer 1

Answer:

(3) X(g) + Y2 (g) ---> XY2 (g)

Explanation:

Here, in the stated gaseous reaction, the Volume of the container (insulated and sealed container) and the pressure of the reaction (given) remains constant.

So, using Ideal Gas Equation:

n1*T1 = n2*T2 ---- (1)

n1 in Rtn 3 is 2 and n2 is 1.

Putting the values of n1, n2,T1 (200K) and T2(400K), the equation 1 is satisfied only for reaction 3. So, reaction 3 is the answer.

Answer 2

The correct answer to the above question is (4) and the explanation is given below.

• Since when a temperature increases from 200K to 400K, this signifies that the reaction which was carried out is the exothermic reaction.. Exothermic reactions are those which release heat energy which causes a rise in temperature. So the reaction should be the formation reaction.
• As given in the question, that pressure remains the same, so the number of moles of reactant should be equal to the number of moles of product. So that reaction that has the same mole in the reactant, as well as product side will be the correct answer.
• So the equation which fulfills the condition is 4, which is X₂ + Y₂→ 2XY.

So the correct option is (4) which is X₂ + Y₂→ 2XY.