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JEE MainChemistrySome Basic Concepts of Chemistry

Consider the unbalanced combustion reaction of propane: C ₃ H ₈(g) + O ₂(g) CO ₂(g) + H ₂ O (l) Which of the following statements is correct?

Options

  1. A67.2 L of CO ₂(g) at STP is produced for every mole of C ₃ H ₈(g) consumed.
  2. B89.6 L of H ₂ O (l) at STP is produced for every mole of C ₃ H ₈(g) consumed.
  3. C22.4 L of CO ₂(g) at STP is produced for every mole of C ₃ H ₈(g) consumed.
  4. D13.44 L of CO ₂(g) is produced regardless of temperature and pressure for every mole of O ₂(g) consumed.

Correct answer

A. 67.2 L of CO ₂(g) at STP is produced for every mole of C ₃ H ₈(g) consumed.

Step-by-step solution

First, balance the chemical equation: C ₃ H ₈(g) + 5 O ₂(g) 3 CO ₂(g) + 4 H ₂ O (l) Checking each option: For every 1 mole of C ₃ H ₈(g) consumed, 3 moles of CO ₂(g) are produced. At STP, the volume of CO ₂(g) is 3 22.4 L = 67.2 L . This makes the first statement correct. For every 1 mole of C ₃ H ₈(g) , 4 moles of H ₂ O (l) are produced. Since water is a liquid at STP, its volume cannot be calculated using the molar volume of a gas ( 22.4 L mol ⁻¹ ). The statement claiming 22.4 L of CO ₂(g) is produced assumes an

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