Consider the reaction. 2 HBr(g) ¡ H2(g) + Br2(g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. b. In the first 25.0 s of this reaction, the concentration of HBr drops from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval. c. If the volume of the reaction vessel in part b is 1.50 L, what amount of Br2 (in moles) forms during the first 15.0 s of the reaction?

Answer :

(A) The rate expression will be:

(B) The average rate of the reaction during this time interval is, 0.00176 M/s

(C) The amount of Br₂ (in moles) formed is, 0.0396 mol

Explanation :

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The given rate of reaction is,

The expression for rate of reaction :

Part A:

The rate expression will be:

Part B:

The average rate of the reaction during this time interval is, 0.00176 M/s

Part C:

As we are given that the volume of the reaction vessel is 1.50 L.

Now we have to determine the amount of Br₂ (in moles).

The amount of Br₂ (in moles) formed is, 0.0396 mol

it is a solid

explanation: