Question

The decomposition of A into product has value of k as 4.5 × 103 s−1 at 10°C and energy of activation 60 kJ mol−1. At what temperature would k be 1.5 × 104 s−1?

Answer 1

Hey Dear,

◆ Answer -

k would be 1.5×10^4 at 297 K

● Explanation -

# Given -

T1 = 10 ℃ = 283 K

Ea = 60 kJ/mol = 6×10^4 J/mol

k1 = 4.5×10^3 s^-1

k2 = 1.5×10^4 s^-1

# Solution -

We know the famous Arrhenius equation,

logk = logA - Ea / 2.303RT

It can be modified for various temperatures as -

log(k2/k1) = Ea(T2-T1) / (2.303R.T1.T2)

Substitute values,

log(1.5×10^4/4.5×10^3) = 6×10^4 (T2-283) / [2.303×8.314×283×T2]

0.5229 = 11.07 × (T2-283)/T2

1 - 283/T2 = 0.0472

T2 = 283 / (1-0.0472)

T2 = 297 K

Thus, k would be 1.5×10^4 at 297 K.

Thanks dear...

Answer 2

Explanation:

answer is in the pic

hope it will help

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