The rate constant for first-order degradation of a N2O2 in a solution (1.0 mg/ml) at 40°C
is 0.00351 hr-1, activation energy is 2000 cal/mol, and R = 1.987 cal/mol/degree.
Calculate
a. The rate constant for first-order degradation of N2O2 at room temperature (25°C).

Question

04-11-2022
Mathematics

Answered

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The rate constant for first-order degradation of a N2O2 in a solution (1.0 mg/ml) at 40°C
is 0.00351 hr-1, activation energy is 2000 cal/mol, and R = 1.987 cal/mol/degree.
Calculate
a. The rate constant for first-order degradation of N2O2 at room temperature (25°C).

Sagot :

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The rate constant for first-order degradation of a N2O2 in a solution (1.0 mg/ml) at 40°C is 0.00351 hr-1, activation energy is 2000 cal/mol, and R = 1.987 cal/mol/degree.Calculate a. The rate constant for first-order degradation of N2O2 at room temperature (25°C).​

Sagot :

Other Questions

The rate constant for first-order degradation of a N2O2 in a solution (1.0 mg/ml) at 40°C
is 0.00351 hr-1, activation energy is 2000 cal/mol, and R = 1.987 cal/mol/degree.
Calculate
a. The rate constant for first-order degradation of N2O2 at room temperature (25°C).