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Textbook Solution:

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Answer:

Interpretation Introduction

a$a$

Interpretation:

To write the expression of rate from the given statement of a chemical reaction.

Concept introduction:

Rate of a chemical reaction: It tells us about the speed at which the reactants are converted into products.

Mathematically, rate of reaction is directly proportional to the product of concentration of each reactant raised to the power equal to their respective stoichiometric coefficients.

Let’s say we have a reaction:

                                    aA+bB−→−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−−cC+dDthen,                                            rate α [A]a[B]b                                      ⇒rate =Kf [A]a[B]bwhere Kf= rate constanta and b are order of reaction with respect to A and B $\begin{array}{l}\text{aA+bB}\stackrel{}{\to }\text{cC+dD}\\ \text{then,}\\ \text{rate}\text{α}{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}\\ \Rightarrow \text{rate}{\text{=K}}_{\text{f}}{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}\\ \text{where}{\text{K}}_{\text{f}}\text{= rate}\text{constant}\\ \text{a and b are order of reaction with respect to A and B }\\ \end{array}$

Answer

Expression of rate is:

                         rate = k[NH3]0 =⇒===============                            rate = k$\begin{array}{l}\text{rate}\text{=}{\text{k[NH}}_{\text{3}}{\text{]}}^0\\ \Rightarrow \text{rate}\text{=}\text{k}\end{array}$

Explanation

Ammonia decomposes into nitrogen and hydrogen gas as:

       2NH3 (g)−→−−−tungsten N2(g) + 3H2 (g)$2{\text{NH}}_{\text{3}}\text{(g)}\stackrel{tungs\mathrm{t}en}{\to }{\text{N}}_{\text{2}}\text{(g)}\text{+}3{\text{H}}_{\text{2}}\text{(g)}$

Since the order of reaction with respect to NH3 is ZERO. Thus, rate law equation will look like:

            2NH3 (g)−→−−−tungsten N2(g) + 3H2 (g)                         rate = k[NH3]0 =⇒========================                            rate = k