Question

the rate of a reaction triples when temperature changes from 20 degree Celsius to 50 degree Celsius calculate the energy of activation​

Answer 1

We shall use arrhenius equation

log k₂/k₁ =Ea/2.303RT (1/T₁ - 1/T₂)

log 3 = Ea/2.303 x 8.314 ( 1/293 - 1/373)

0.477 = Ea/19.147 ( 7.34 x 10^-4)

0.477 = 0.014 Ea

Ea = 34 kJmol⁻¹

Ea is the activation energy.

I hope it helps you.

Answer 2

Answer:

Explanation:According to Arrhenius equation,

Log k2/k1=Ea/2.303R (T2-T1/T1*T2)

T1= 20 degree Celsius = 20+273=293 K

T2= 50 degree celsius=50+273= 323K

Log3= Ea/2.303*8.314JK-1mol-1(323-293)/293*323

0.4771= Ea*30/2.303*8.314*293*323

0.4771*2.303*8.314*293*323/30= Ea

Ea = 28817.8955318733JK-1mol-1

Ea = 28.82KJmol-1