Use the value of the activation energy (Ea=1.50×102kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.

The rate constant

K= 0.967m-1s-1

Explanation: To calculate the rate constant, we will use the Arrhenius equation.

lnK = (- Ea/R) (1/T) + lnZ(1)

K is the rate constant

Ea is the activation energy

R is the gas constant

T is the temperature in Kelvin

Z is the constant related to the geometry needed, but in this question Z is equal to zero.

Therefore fro data given, we have

Ea = 1.50 × 102kj/mol = 153kj/mol

R = 8.314j/mol-k

T = 551k

Z= 0

Therefore using the equation

lnK = -153÷ (8.314 × 551) = -153 × 4581.014

lnK = - 0.033398719

Taking the ln inverse of K

K = e^ (-0.033398819) = 0.96715286

K= 0.967m-1s-1

This is the rate constant

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