At a certain time in a reaction, substance a is disappearing at a rate of 4.0×10−2 m/s, substance b is appearing at a rate of 2.0×10−2 m/s, and substance c is appearing at a rate of 6.0×10−2 m/s. which of the following could be the stoichiometry for the reaction being studied?

Answer : The required equation will be:

Explanation :

Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

As we are given that:

Rate of disappearing component A =

Rate of appearing component B =

Rate of appearing component C =

The general reaction is:

As per question the stoichiometry relation will be:

Now put the values of rate of following components, we get:

Thus, the stoichiometry relation is:

a : b : c = 2 : 1 : 3

Thus, the required equation will be:

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.