. 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

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.

6.4 cm (max) - 25 cm (min)