1 mole of PbS is oxidised by “X” moles of O3>to get “Y” moles of O2. X + Y = __________
Correct Answer: 8
Approach Solution - 1
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].
Approach Solution -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
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