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In the reaction : 2N₂O₅ → 4NO₂ + O₂, initial pressure is 500 atm and rate constant k is 3.38 ˣ 10⁻⁵ s⁻¹.After 10 minutes the final pressure of N₂O₅ is
Options
(a) 490 atm
(b) 250 atm
(c) 480 atm
(d) 420 atm
Correct Answer:
490 atm
Explanation:
P₀ = 500 atm. k = 2.303 / t log₁₀ p₀ / p(t), 3.38 ⨯ 10⁻⁵ = 2.303 / 10⨯60 log 500/ p(t) or, 0.00880 = log 500 / p(t) ⇒ 500 / 1.02 = 490 atm.
Related Questions: - Using the Gibb’s energy change,ΔG⁰ = +63.3 kJ, for the following reaction
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Topics: Electrochemistry and Chemical Kinetics
(87)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Using the Gibb’s energy change,ΔG⁰ = +63.3 kJ, for the following reaction
- The crystal structure of solid Mn(II) oxide is
- Which one gives secondary alcohol when treated with Grignard reagent
- Which of the following has zero valency
- Different gases at the same temperature must have
Topics: Electrochemistry and Chemical Kinetics (87)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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