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The difference between ΔH and ΔE at 300 K for the reaction
C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(l)
Options
(a) 300 ˣ 8.31 J/mol
(b) -300 ˣ 8.314 J/mol
(c) 3 ˣ 300 ˣ 8.314 J/mol
(d) -3 ˣ 300 ˣ 8.314 J/mol
Correct Answer:
-3 ˣ 300 ˣ 8.314 J/mol
Explanation:
ΔH = ΔE + Δn(g)RT
or ΔH – ΔE = Δn(g)RT,
where Δn(g) = (3) – (5 + 1) = -3.
Thus, ΔH – ΔE = -3 * 8.31 *300 J/mol.
Related Questions: - Which one of the following is a false statement
- If the value of an equilibrium constant for a particular reaction is 1.6 ˣ 10¹²,
- Which one of the following is not an amphoteric substance
- When acetic acid is heated with phosphorus pentaoxide(P₂O₅), the compound
- How enzymes increases the rate of reaction
Topics: Thermodynamics
(179)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Which one of the following is a false statement
- If the value of an equilibrium constant for a particular reaction is 1.6 ˣ 10¹²,
- Which one of the following is not an amphoteric substance
- When acetic acid is heated with phosphorus pentaoxide(P₂O₅), the compound
- How enzymes increases the rate of reaction
Topics: Thermodynamics (179)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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