# Write the rates for the following reactions in terms of the disappearance of reactants and...

## Question:

Write the rates for the following reactions in terms of the disappearance of reactants and appearance of products.

a. 3O{eq}_2 {/eq} {eq}\rightarrow {/eq} 2O{eq}_3 {/eq}

b. C{eq}_2 {/eq}H{eq}_6 {/eq} {eq}\rightarrow {/eq} C{eq}_2 {/eq}H{eq}_4 {/eq} + H{eq}_2 {/eq}

c. ClO{eq}^- {/eq} + Br{eq}^- {/eq} {eq}\rightarrow {/eq} BrO{eq}^- {/eq} + Cl{eq}^- {/eq}

d. (CH{eq}_3 {/eq}){eq}_3 {/eq}CCl + H{eq}_2 {/eq}O {eq}\rightarrow {/eq} (CH{eq}_3 {/eq}){eq}_3 {/eq}COH + H{eq}^+ {/eq} + Cl{eq}^- {/eq}

e. 2AsH{eq}_3 {/eq} {eq}\rightarrow {/eq} 2As + 3H{eq}_2 {/eq}

## Rate of Reaction

Rate of a reaction can be expressed in terms of the amount of reactants or products. Since a reactant decreases in amount as the reaction progresses, the rate expression of a reaction expressed using the amount of reactants would have a negative sign but a positive sign if it is expressed in terms of a product.

a) {eq}3O_2 \rightarrow 2O_3 {/eq}

{eq}rate = - \dfrac {1}{3} \dfrac { \Delta [O_2] }{ \Delta t } = \dfrac {1}{2} \dfrac { \Delta [O_3] }{ \Delta t...

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