Question

Determine the rate of chemical reaction proceeding according to the scheme
3А + 2В > 2С + 3D. Concentration of substance А is 9.0 mol/l, of substance В is
0.6 mol/l, rate constant is 0.9 mol/l·min.

Answer 1

Answer:

rate of given chemical reaction is 236.20

Explanation:

according to rate law

Rate = k[A]³[B]²

Answer 2

Answer:

Learning Objectives

By the end of this section, you will be able to:

Explain the form and function of a rate law

Use rate laws to calculate reaction rates

Use rate and concentration data to identify reaction orders and derive rate laws

As described in the previous module, the rate of a reaction is affected by the concentrations of reactants. Rate laws or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. In general, a rate law (or differential rate law, as it is sometimes called) takes this form:

rate=k[A]m[B]n[C]p…rate=k[A]m[B]n[C]p…

in which [A], [B], and [C] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature. The exponents m, n, and p are usually positive integers (although it is possible for them to be fractions or negative numbers). The rate constant k and the exponents m, n, and p must be determined experimentally by observing how the rate of a reaction changes as the concentrations of the reactants are changed. The rate constant k is independent of the concentration of A, B, or C, but it does vary with temperature and surface area.

The exponents in a rate law describe the effects of the reactant concentrations on the reaction rate and define the reaction order. Consider a reaction for which the rate law is:

rate=k[A]m[B]nrate=k[A]m[B]n

If the exponent m is 1, the reaction is first order with respect to A. If m is 2, the reaction is second order with respect to A. If n is 1, the reaction is first order in B. If n is 2, the reaction is second order in B. If m or n is zero, the reaction is zero order in A or B, respectively, and the rate of the reaction is not affected by the concentration of that reactant. The overall reaction order is the sum of the orders with respect to each reactant. If m = 1 and n = 1, the overall order of the reaction is second order (m + n = 1 + 1 = 2).

The rate law:

rate=k[H2O2]rate=k[H2O2]

describes a reaction that is first order in hydrogen peroxide and first order overall. The rate law:

rate=k[C4H6]2rate=k[C4H6]2

describes a reaction that is second order in C4H6 and second order overall. The rate law:

rate=k[H+][OH−]rate=k[H+][OH−]

describes a reaction that is first order in H+, first order in OH−, and second order overall.

Example 1

Writing Rate Laws from Reaction Orders

An experiment shows that the reaction of nitrogen dioxide with carbon monoxide:

NO2(g)+CO(g)⟶NO(g)+CO2(g)NO2(g)+CO(g)⟶NO(g)+CO2(g)

is second order in NO2 and zero order in CO at 100 °C. What is the rate law for the reaction?

Solution

The reaction will have the form:

rate=k[NO2]m[CO]nrate=k[NO2]m[CO]n

The reaction is second order in NO2; thus m = 2. The reaction is zero order in CO; thus n = 0. The rate law is:

rate=k[NO2]2[CO]0=k[NO2]2rate=k[NO2]2[CO]0=k[NO2]2

Remember that a number raised to the zero power is equal to 1, thus [CO]0 = 1, which is why we can simply drop the concentration of CO from the rate equation: the rate of reaction is solely dependent on the concentration of NO2. When we consider rate mechanisms later in this chapter, we will explain how a reactant’s concentration can have no effect on a reaction despite being involved in the reaction.

Check Your Learning

The rate law for the reaction:

H2(g)+2NO(g)⟶N2O(g)+H2O(g)H2(g)+2NO(g)⟶N2O(g)+H2O(g)

has been determined to be rate = k[NO]2[H2]. What are the orders with respect to each reactant, and what is the overall order of the reaction