Enter your answer in the provided box. remember to enter your answer to the correct number of significant figures. for the reaction: a(g) + b(g) → ab(g) the rate is 0.23 mol/l·s, when [a]0 = [b]0 = 1.0 mol/l. if the reaction is first order in b and second order in a, what is the rate when [a]0 = 2.0 mol/l and [b]0 = 4.6 mol/l?

Answer : The rate law is 4.232 mol/L.s

Explanation :

First we have to calculate the value of rate constant.

According to the question, the expression for rate law will be:

where,

k = rate constant

As we are given :

Rate law = 0.23 mol/L.s

Initial concentration of A = 1.0 mol/L

Initial concentration of B = 1.0 mol/L

Now put all the given values in the above rate law expression, we get:

Now we have to calculate the rate law when initial concentration of A and B is 2.0 mol/L and 4.6 mol//L respectively.

The expression for rate law will be:

where,

k = rate constant =

Rate law = ?

Initial concentration of A = 2.0 mol/L

Initial concentration of B = 4.6 mol/L

Now put all the given values in the above rate law expression, we get:

Therefore, the rate law is 4.232 mol/L.s

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every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.