Question

An industrial chemical reaction has a rate law: rate = k [C]. the activation energy for the reaction is 3.0000*10^4 J/mol and A= 2.000*10^-3. What must be the reaction temperature is a rate of 1.00*10^-9M/s is required and [C] must be kept at 0.0300M?

Answer 1

a) Given that rate = k[C]

1.00 x 10^-9 M/s = k x  0.0300M

k = 3.33 x 10^-8 s^-1

b)

Arrhenius equation is

Arrhenius equation k = A e^-Ea/RT

Given that

k = rate of reaction =   3.33 x 10^-8 s^-1

A = collision frequency = 2.000*10^-3

Ea = activation energy = 3.0000*10^4 J/mol

R= universal gas constant = 8.314 J/K/mol

T = temperature = ?

k = A e^-Ea/RT

3.33 x 10^-8 s^-1 = ( 2.0 x10^-3) e^ [- 3.0 x10⁴ J/mol/ (8.314 J/K/mol ) (T) ]

On solving,

T = 327.9 K

Therefore,

required temperature = 327.9 K