Acertain first-order reaction has a rate constant of 2.75 10-2 s−1 at 20.°c. what is the value of k at 45°c if ea = 75.5 kj/mol? webassign will check your answer for the correct number of significant figures. 0.0352 incorrect: your answer is incorrect.

The value of (rate constant) will be 0.314 s⁻¹  at 45°C if activation energy is 75.5 kJ/mol.

It describes the effect of temperature change on the rate of reaction.

Where,

k₁ - rate constant = 0.0275 s⁻¹            

k₂ = ?

Eₐ - Activation energy = 75.5 kJ·mol⁻¹

T₁- Initial temperature = 20 °C = 293.15 K

T₂- Final temperature = 45°C = 318.15 K

Put the values in the formula,

Therefore, the value of (rate constant) will be 0.314 s⁻¹  at 45°C if activation energy is 75.5 kJ/mol.

Learn more about Arrhenius equation:

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0.314 s⁻¹  

Step-by-step explanation:

Use the Arrhenius equation.

Data:

k₁ = 0.0275 s⁻¹;            k₂ = ?

Eₐ = 75.5 kJ·mol⁻¹

T₁ = 20 °C = 293.15 K; T₂ = 45°C = 318.15 K

Calculation:

k₂ = 0.0275 × 11.41

k₂ = 0.314 s⁻¹

the answer is true.