Home
Class 12
CHEMISTRY
The energy of activation for a first ...

The energy of activation for a first order reaction is 104 kJ `mol^(-1) ` The rate constant at `25^(@) C` is `3.7 xx 10^(-5) s^(-1)` . What is the rate constant at `30^(@) C`

Text Solution

Verified by Experts

The correct Answer is:
Rate constant at `30^(@) C = 7.4 xx 10^(-4) s^(-1)`
Given : Energy of activation `=E_(a) =104 kJ mol^(-1) = 104 xx 10^(3) j mol^(-1)`
Initial rate constant = `k_(1) = 3.7 xx 10^(-5) s^(-1)`
Initial temperature = `T_(1)= 273 + 25 = 298 K`
Final temperature =`T_(2) = 273 + 30 = 303 K`
Final rate constant = `k_(2) = ?`
`log_(10) .(k_(2))/(k_(1)) = (E_(a) (T_(2)- T_(1)))/(2.303 R xx T_(1) xx T_(2))`
`= (104xx 10^(3) xx (303 - 298))/(2.303 xx 8.314 xx 298 xx 303) = (104 xx 10^(5) xx 5)/(2.303 xx 8.314 xx298 xx 303) =0.3`
`:. (k_(2))/(k_(1)) = AL 0.3 = 1.995 ~= 2`
`:. k_(2) = 2 xx k_(1) = 2xx 3.7 xx 10^(-5) = 7.4 xx 10^(-4) s^(-1)`
Promotional Banner

Similar Questions

Explore conceptually related problems

The energy of activation of a first order reaction is 187.06 kJ mol^(-1) at 750 K and the value of pre-exponential factor A is 1.97xx10^(12)s^(-1) . Calculate the rate constant and half life. (e^(-30)= 9.35xx10^(-14))

The energy of activation of a reaction is 140 kJ "mol"^(-1) . If its rate constant at 400 K is 2.0xx10^(-6) s^(-1) , what is the value at 500 K

The activation energy of a reaction is 94.14 kJ mol^(-1) and the value of rate constant at 313 K is 1.8 xx 10^(-5)s^(-1) . Calculate the frequency factor A.

The activation energy of a reaction is 94.14 "kJ mol"^(-1) and the value of rate constant at 313 K is 1.8xx10^(-5) s^(-1) . Calculate the frequency factor A

The activation energy of a reaction is 94.14 kJ mol^(-1) and the value of rate constant at 313 K is 18 xx 10^(-5) s^(-1) . Calculate the frequency factor or pre-exponential factor, A .

The rate constant for a first order reaction at 300^(@)C for which E_(a) is 35 kcal mol^(-1) and frequency constant is 1.45 xx 10^(11) s^(-1) is

The reaction 2NO_(2)rarr2NO+O_(2) has an activation energy of 110 KJ mol^(-) . At 400^(@)C , the rate constant is 7.8mol^(-1)Ls^(-1) . What is the value of rate constant at 430^(@)C ?

For a chemical reaction the energy of activation is 85 kJ "mol"^(-1) If the frequency factor is 4.0xx10^(9) L "mol"^(-1)s^(-1) , what is the rate constant at 400 K?