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The gas-phase reaction 2 N₂O5 (g) → 4 NO₂ (g) + O₂(g) has an activation energy of 103 kJ/mol, and the rate constant is 0.0900 min-¹ at 328.0 K. Find the rate constant at 313.8 K. The value of gas constant is 8.3145 x 103 kJ/K . mol. Rate constant = min -1

The gas-phase reaction 2 N₂O5 (g) → 4 NO₂ (g) + O₂(g) has an activation energy of 103 kJ/mol, and the rate constant is 0.0900 min-¹ at 328.0 K. Find the rate constant at 313.8 K. The value of gas constant is 8.3145 x 103 kJ/K . mol. Rate constant = min -1

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter16: Reaction Rates
Section16.3: Reaction Rate Laws
Problem 26SSC
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The gas-phase reaction 2 N₂O5 (g) → 4 NO₂ (g) + O2 (g) has an activation energy of 103 kJ/mol, and the rate constant is 0.0900 min-1 at 328.0 K. Find the rate constant at 313.8 K. The value of gas constant is 8.3145 × 10-³ kJ/K - mol. Rate constant = min-1
Transcribed Image Text:The gas-phase reaction 2 N₂O5 (g) → 4 NO₂ (g) + O2 (g) has an activation energy of 103 kJ/mol, and the rate constant is 0.0900 min-1 at 328.0 K. Find the rate constant at 313.8 K. The value of gas constant is 8.3145 × 10-³ kJ/K - mol. Rate constant = min-1
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