Write rate equations for each of the following reaction: Cyclopropane → propene (where rate is proportional to the concentration of cyclopropane)

Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [reactant ] For the reaction, Cyclopropane → propene The rate is proportional to the concentration of cyclopropane. Therefore, the rate equation is as follows Rate = k [ cyclopropane ]

Write rate equations for each of the following reaction: Cyclopropane → propene (where rate is proportional to the concentration of cyclopropane)

Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [reactant ] For the reaction, Cyclopropane → propene The rate is proportional to the concentration of cyclopropane. Therefore, the rate equation is as follows Rate = k [ cyclopropane ]

Write rate equations for each of the following reaction: 2 HI ( g ) → H 2 ( g ) + I 2 ( g ) where rate is proportional to the square of the hydrogen iodide concentration.

Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [reactant ] n For the reaction, 2 HI ( g ) → H 2 ( g ) + I 2 ( g ) The rate is proportional to the square of the concentration of hydrogen iodide. Therefore, the rate equation is as follows Rate = k [ HI ] 2

Write rate equation for the following reaction: C 12 H 22 O 11 ( g ) + H 2 O ( l ) → H + 2 C 6 H 12 O 6 ( aq ) where rate is proportional to the concentration of C 12 H 22 O 11 and to the concentration of H + ions.

Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [reactant] n For the reaction, C 12 H 22 O 11 ( g ) + H 2 O ( l ) → H + 2 C 6 H 12 O 6 ( aq ) The rate is proportional to the concentration of C 12 H 22 O 11 and H + . Therefore, the rate equation is as follows Rate = k C 12 H 22 O 11 H +

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction. 2 HI ( g ) → H 2 ( g ) + I 2 ( g ) where rate is proportional to the square of the hydrogen iodide concentration.

The order of the reaction can be determined by the rate equation. Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [ reactant ] n where n represents the order of reaction. For the reaction, 2 HI ( g ) → H 2 ( g ) + I 2 ( g ) The rate is proportional to the square of the concentration of hydrogen iodide. Therefore, the rate equation is as follows Rate = k [ HI ] 2 As evident from the rate law expression, the reaction is second order with respect to hydrogen iodide and overall second order.

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction. C 12 H 22 O 11 ( g ) + H 2 O ( l ) → H + 2 C 6 H 12 O 6 ( aq ) where rate is proportional to the concentration of C 12 H 22 O 11 and to the concentration of H + ions.

The order of the reaction can be determined by the rate equation. Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [ reactant ] n where n represents the order of reaction. For the reaction, C 12 H 22 O 11 ( g ) + H 2 O ( l ) → H + 2 C 6 H 12 O 6 ( aq ) The rate is proportional to the square of the concentration of C 12 H 22 O 11 and H + . Therefore, the rate equation is as follows Rate = k C 12 H 22 O 11 H + As evident from the rate law expression, the reaction is first order with respect to C 12 H 22 O 11 and first order with respect to H + , overall it is a second order reaction.

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction. 2 HgCl 2 ( aq ) + K 2 C 2 O 4 ( aq ) → Hg 2 Cl 2 ( s ) + 2 KCl ( aq ) + 2 CO 2 ( g ) where rate is proportional to the concentration of HgCl 2 and to the square of the concentration of K 2 C 2 O 4 .

The order of the reaction can be determined by the rate equation. Rate equation is a mathematical description of a reaction's rate as a function of the concentration of the reactants, and the rate constant ( k ) . Usually in a form similar to rate = k [ reactant ] n where n represents the order of reaction. For the reaction, 2 HgCl 2 ( aq ) + K 2 C 2 O 4 ( aq ) → Hg 2 Cl 2 ( s ) + 2 KCl ( aq ) + 2 CO 2 ( g ) The rate is proportional to the concentration of HgCl 2 and to the square of the concentration of K 2 C 4 O 4 . Therefore, the rate equation is as follows Rate = k HgCl 2 K 2 C 2 O 4 2 As evident from the rate law expression, the reaction is first order with respect to HgCl 2 and second order with respect to K 2 C 2 O 4 and overall it is a third order reaction.

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AS and A Level

IMPORTANT

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Write rate equations for each of the following reaction:

Cyclopropane $\to$ propene (where rate is proportional to the concentration of cyclopropane)

Important Questions on Reaction Kinetics

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 1

Write rate equations for each of the following reaction:

$2 HI (g) \to H_{2} (g) + I_{2} (g)$ where rate is proportional to the square of the hydrogen iodide concentration.

HARD

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 1

Write rate equation for the following reaction:

$C_{12} H_{22} O_{11} (g) + H_{2} O (l) \overset{H^{+}}{\to} 2 C_{6} H_{12} O_{6} (aq)$ where rate is proportional to the concentration of $C_{12} H_{22} O_{11}$ and to the concentration of $H^{+}$ ions.

MEDIUM

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 1

Write rate equations for each of the following reaction:

$2 {HgCl}_{2} (aq) + K_{2} C_{2} O_{4} (aq) \to {Hg}_{2} {Cl}_{2} (s) + 2 KCl (aq) + 2 {CO}_{2} (g)$ where rate is proportional to the concentration of ${HgCl}_{2}$ and to the square of the concentration of $K_{2} C_{2} O_{4}$ .

MEDIUM

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 1

Write rate equations for each of the following reaction:

${CH}_{3} {COCH}_{3} + I_{2} \overset{H^{+}}{\to} {CH}_{3} {COCH}_{2} I + HI$ where rate is proportional to the concentration of ${CH}_{3} {COCH}_{3}$ and to the concentration of $H^{+}$ ions, but the concentration of $I_{2}$ has no effect on the rate.

HARD

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 2

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction.

Cyclopropane $\to$ propene (where rate is proportional to the concentration of cyclopropane)

HARD

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 2

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction.

$2 HI (g) \to H_{2} (g) + I_{2} (g)$ where rate is proportional to the square of the hydrogen iodide concentration.

HARD

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 2

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction.

MEDIUM

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 22 - Reaction Kinetics>Question>Q 2

For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction.

Write rate equations for each of the following reaction: Cyclopropane → propene (where rate is proportional to the concentration of cyclopropane)

Important Questions on Reaction Kinetics

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Write rate equations for each of the following reaction:

Cyclopropane $\to$ propene (where rate is proportional to the concentration of cyclopropane)