Question

1 mole of PbS is oxidised by “X” moles of O₃>to get “Y” moles of O2. X + Y = __________

Answer 1

Correct Answer: 8

To solve this problem, we need to determine the number of moles of O₃ and O₂ involved when 1 mole of PbS is oxidized. The chemical reaction for oxidizing PbS using O₃ is:

PbS + 4O₃ → PbSO₄ + 4O₂ 

Step-by-step explanation:

From the balanced reaction, 1 mole of PbS requires 4 moles of O₃ to be oxidized to PbSO₄.

During this process, it produces 4 moles of O₂.

Given these stoichiometric relationships, the number of moles of O₃ (“X” moles) used is 4, and the number of moles of O₂ (“Y” moles) produced is also 4.

The problem asks for the sum X + Y, which is:

X + Y = 4 + 4 = 8

Verification:

The computed value of X + Y = 8 falls within the expected range of [8,8].

Answer 2

The balanced chemical equation for the oxidation of PbS by ozone is:

\(\text{PbS} + 4\text{O}_3 \rightarrow \text{PbSO}_4 + 4\text{O}_2\)

From the equation:
- 1 mole of PbS reacts with 4 moles of \( \text{O}_3 \), so \( X = 4 \).
- 4 moles of \( \text{O}_2 \) are produced, so \( Y = 4 \).

Therefore:

\(X + Y = 4 + 4 = 8\)

The Correct answer is: 8