For the reaction; 4 NH3( g)+5 O2( g) ⟶4 NO(g)+6 H2 O(g), the rate of reaction in terms of disapp

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For the reaction; 4 NH3( g)+5 O2( g) ⟶4 NO(g)+6 H2 O(g), the...

For the reaction; $4 \mathrm{NH}_{3(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}$, the rate of reaction in terms of disappearance of $\mathrm{NH}_{3}$ is $-\frac{d\left[\mathrm{NH}_{3}\right]}{d t}$, then write the rate expression in terms of concentration of $\mathrm{O}_{2}, \mathrm{NO}$ and $\mathrm{H}_{2} \mathrm{O}$

For the reaction; $4 \mathrm{NH}_{3(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}$, the
rate of reaction in terms of disappearance of $\mathrm{NH}_{3}$ is $-\frac{d\left[\mathrm{NH}_{3}\right]}{d t}$, then write the rate expression in terms of concentration of $\mathrm{O}_{2}, \mathrm{NO}$ and $\mathrm{H}_{2} \mathrm{O}$

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Key Concepts

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the mole ratios of reactants and products. This allows conversion between the rate of disappearance of one component and the rate of appearance of another by taking into account the stoichiometric coefficients from the reaction equation.

Rate of Reaction

The rate of reaction is defined as the change in concentration of a reactant or product over time. For reactants, the rate is expressed as a negative change in concentration per unit time, while for products, it is positive. This indicates how fast the reactant is being consumed or the product is formed.

Rate Expression

A rate expression mathematically represents the rate of a reaction in terms of the concentration of one or more reactants and products. By incorporating the stoichiometric factors, the rate expression accounts for the proportional changes in concentration of each species relative to the overall reaction rate, ensuring consistency across the reaction.

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