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 × 10⁴s^–1?

Question

The decomposition of A into product has value of k as 4.5 × 10 3 s –1 at 10°C and energy of activation 60 kJ mol –1 . At what temperature would k be 1.5 × 10 4 s –1 ?

Philoid · Accepted Answer

From Arrhenius equation, we obtain

Also, k₁ = 4.5 × 10³ s ^{- 1}

T₁ = 273 + 10 = 283 K

k₂ = 1.5 × 10⁴ s ^{- 1}

E_a = 60 kJ mol ^{- 1} = 6.0 × 10⁴ J mol ^{- 1}

Then,

→ 0.5229 = 3133.627 × (T₂-283)/(283 × T₂)

→ 0.0472T₂ = T₂-283

T₂ = 297K or T₂ = 24⁰ C

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 × 104s–1?

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 × 10⁴s^–1?