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If rate of formation of SO3 is 0.8 g.lit–1.sec–1 then calculate the rate of disappearance of O2 in g.lit–1.sec–1 for the reaction 2SO2 + O2 → 2SO3
Correct answer is '0.16'. Can you explain this answer?
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If rate of formation of SO3is 0.8 g.lit–1.sec–1then calcul...
Understanding the Reaction
The chemical reaction involved is:
\[ 2 \text{SO}_2 + \text{O}_2 \rightarrow 2 \text{SO}_3 \]
This indicates that for every 2 moles of sulfur dioxide (SO2) consumed, 1 mole of oxygen (O2) is consumed, resulting in the formation of 2 moles of sulfur trioxide (SO3).
Rate of Formation and Disappearance
Given the rate of formation of SO3:
- Rate of formation of SO3 = 0.8 g.lit-1.sec-1
From the stoichiometry of the reaction, we can derive the rate of disappearance of O2.
Stoichiometric Relationships
- According to the reaction:
- 2 moles of SO2 react with 1 mole of O2 to produce 2 moles of SO3.
- Therefore, the rate of disappearance of O2 is related to the rate of formation of SO3 by the following ratio:
- For every 2 moles of SO3 formed, 1 mole of O2 is consumed.
Calculating the Rate of Disappearance of O2
- Using the stoichiometric coefficients:
\[
\text{Rate of disappearance of O}_2 = \frac{1}{2} \times \text{Rate of formation of SO}_3
\]
- Substituting the given value:
\[
\text{Rate of disappearance of O}_2 = \frac{1}{2} \times 0.8 \, \text{g.lit}^{-1}\text{.sec}^{-1} = 0.4 \, \text{g.lit}^{-1}\text{.sec}^{-1}
\]
- Since we are considering the rate of O2 disappearance per mole formation of SO3, we need to divide by 2 again:
\[
\text{Rate of disappearance of O}_2 = \frac{0.4}{2} = 0.16 \, \text{g.lit}^{-1}\text{.sec}^{-1}
\]
Conclusion
Thus, the rate of disappearance of O2 is confirmed as:
- 0.16 g.lit-1.sec-1.
The chemical reaction involved is:
\[ 2 \text{SO}_2 + \text{O}_2 \rightarrow 2 \text{SO}_3 \]
This indicates that for every 2 moles of sulfur dioxide (SO2) consumed, 1 mole of oxygen (O2) is consumed, resulting in the formation of 2 moles of sulfur trioxide (SO3).
Rate of Formation and Disappearance
Given the rate of formation of SO3:
- Rate of formation of SO3 = 0.8 g.lit-1.sec-1
From the stoichiometry of the reaction, we can derive the rate of disappearance of O2.
Stoichiometric Relationships
- According to the reaction:
- 2 moles of SO2 react with 1 mole of O2 to produce 2 moles of SO3.
- Therefore, the rate of disappearance of O2 is related to the rate of formation of SO3 by the following ratio:
- For every 2 moles of SO3 formed, 1 mole of O2 is consumed.
Calculating the Rate of Disappearance of O2
- Using the stoichiometric coefficients:
\[
\text{Rate of disappearance of O}_2 = \frac{1}{2} \times \text{Rate of formation of SO}_3
\]
- Substituting the given value:
\[
\text{Rate of disappearance of O}_2 = \frac{1}{2} \times 0.8 \, \text{g.lit}^{-1}\text{.sec}^{-1} = 0.4 \, \text{g.lit}^{-1}\text{.sec}^{-1}
\]
- Since we are considering the rate of O2 disappearance per mole formation of SO3, we need to divide by 2 again:
\[
\text{Rate of disappearance of O}_2 = \frac{0.4}{2} = 0.16 \, \text{g.lit}^{-1}\text{.sec}^{-1}
\]
Conclusion
Thus, the rate of disappearance of O2 is confirmed as:
- 0.16 g.lit-1.sec-1.
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If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer?
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If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer?.
If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If rate of formation of SO3is 0.8 g.lit–1.sec–1then calculate the rate of disappearance of O2in g.lit–1.sec–1for the reaction 2SO2+ O2→ 2SO3Correct answer is '0.16'. Can you explain this answer?.
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