- 1(current)
Q. No.The first-order rate constant for the decomposition of ethyl iodide by the reaction
C2H5I(g) → C2H4 (g) + HI(g)
at 600K is 1.60 × 10–5 s–1. Its energy of activation is 209 kJ/mol. The rate constant of the reaction at 700K is-
1. 7.56 × 10–3 s–1
2. 6.36 × 10–3 s–1
3. 5.16 × 10–3 s–1
4. 5.76 × 10–3 s–1
Subtopic: Arrhenius Equation |
59%
Level 3: 35%-60%
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What is the pre-exponential factor for a reaction at 500 K with a rate constant of 0.02 s⁻¹ and an activation energy of 18.230 kJ?
1. 1.61
2. 1.41
3. 1.81
4. 1.21
1. 1.61
2. 1.41
3. 1.81
4. 1.21
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
Hints
- 1(current)
Q. No.
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