NEETChemistryChemical Kinetics
The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the value of A is 4 × 10 10 s –1 . Calculate k at 318K and E a
Options
- AE a = 76.750 kJ mol –1 and k = 3.6528 × 10 –2 s –1
- BE a = 86.985 kJ mol –1 and k = 0.9965 × 10 –2 s –1
- CE a = 76.750 kJ mol –1 and k = 0.9965 × 10 –2 s –1
- DE a = 86.985 kJ mol –1 and k = 3.6582 × 10 –2 s –1
Correct answer
C. E a = 76.750 kJ mol –1 and k = 0.9965 × 10 –2 s –1
Step-by-step solution
Correct Option is : (C) E a = 76.750 kJ mol –1 and k = 0.9965 × 10 –2 s –1