The decomposition of A into product has value of k as 4.5×103s-1at 10°C and energy of activation 60 kJ mol-1.
At what temperature would k be 1.5 × 104 s-1
(A) 12°C (B) 24°C (C) 48°C (D) 36°C
(B) k10=k283=4.5×103s-1, kT=1.5×104s-1,T=?Ea=60 kJ mol-1=60,000 J mol-1
Using Arrhenius equation, one can write
logkTk283=Ea2.303 R1283 K-1Tlog1.5×104s-14.5×103s-1=60000J mol-12.303×8.3J K-1mol-1T-283 K283 K×T
On solving this gives T=297K= 24°C