. For 2A + 3B → 2C, [A]0 = 0.15, [B]0 = 0.12, and the initial rate is 0.10 mol/Ls. Assume that the reaction described above is first order in both reactants A and B. Calculate the value of the reaction rate constant.

The rate constant k is ;

K = 2572 L^4/mol^-4•s

Explanation:

In this question, we are asked to calculate the rate constant given the chemical equation above.

First, we need to write a complete expression for the rate law. The reaction is a second order type.

We write the rate law as follows;

Rate = k * [A]^2 * [B]^3

Where k is the rate constant and the square brackets indicate the concentrations of both A and B. Let’s input the values :;

0.1 = k * (0.15)^2 * (0.12)^3

0.1 = k * 0.0225 * 0.001728

0.1 = k * 0.00003888

K = 0.1/0.00003888

K = 2572 L^4/mol^-4•s

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explanation:

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.