Answered

Welcome to Westonci.ca, where your questions are met with accurate answers from a community of experts and enthusiasts. Our platform connects you with professionals ready to provide precise answers to all your questions in various areas of expertise. Get immediate and reliable solutions to your questions from a community of experienced professionals on our platform.

Determine the activation energy for the redox reaction Q²⁺ + 2 R³⁺ → Q⁴⁺ + 2 R²⁺.

Rate Constant Temperature
3.12x10^3 M^-1 s^-1 275K
2.70x10^4 M^-1 s^-1 300K

Sagot :

pstnonsonjoku

The activation energy of the reaction is 6.1 kJ/mol.

What is the Arrhenius equation?

The Arrhenius equation specifies the relationship between the activation energy and the temperature as follows;

ln(k2/k1) = Ea/R(1/T1 - 1/T2)

k1= 3.12x10^3 M^-1 s^-1

k2 = 2.70x10^4 M^-1 s^-1

T1=  275K

T2 = 300K

Hence;

ln(2.70x10^4/3.12x10^3) = Ea/8.314 ×(1/275 - 1/300)

2.2 = 0.0003Ea/8.314

Ea = 2.2 x 8.314/0.0003

Ea = 6.1 kJ/mol

Learn more about activation energy: https://brainly.com/question/11334504

We appreciate your time. Please revisit us for more reliable answers to any questions you may have. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Your questions are important to us at Westonci.ca. Visit again for expert answers and reliable information.