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

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e

where are the choice options?