Draw sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction: 2 HI ( g ) → gold H 2 ( g ) + I 2 ( g ) for which the rate equation is: rate = k Note: the catalyst influences the order here – the order is not the same as for the uncatalysed reaction

The rate of reaction or reaction rate is the speed at which reactants are converted into products. As per the law of mass action, the chemical reaction rate is directly proportional to the concentration of reactants. This implies that the chemical reaction rate increases with the increase in concentration and decreases with the decrease in the concentration of reactants. However, the increase or decrease may be linear as well as non-linear. Furthermore, the rate of the reaction is independent of initial concentration for zero order reactions. For the given reaction ; 2 HI ( g ) → gold H 2 ( g ) + I 2 ( g ) ; Rate = k The order of reaction with respect to HI is zero. So, the reaction rate does not change with concentration of HI , and the plot line is horizontal and straight.

Draw a sketch graph to show how the concentration of the bold reactant changes with time. 2 HI ( g ) → gold H 2 ( g ) + I 2 ( g ) for which the rate equation is: rate = k Note: the catalyst influences the order here – the order is not the same as for the uncatalysed reaction

The reaction rate for a given chemical reaction is the measure of the change in concentration of the reactants or the change in concentration of the products per unit time. With the time, as the concentration of the reactants decreases, the rate of the reaction also decreases accordingly. For the given reaction ; 2 HI ( g ) → gold H 2 ( g ) + I 2 ( g ) ; Rate = k The order of reaction with respect to HI is zero.S0, The reaction proceeds at the same rate whatever the concentration of HI is, and the plot line is descending and straight.

MEDIUM

AS and A Level

IMPORTANT

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State the units of $k$ corresponding to each of the following rate equation:

Rate $= k {[NO]}^{2}$

Important Questions on Reaction Kinetics

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 3

State the units of $k$ corresponding to each of the following rate equation:

Rate $= k {[{NH}_{3}]}^{0}$

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 3

State the units of $k$ corresponding to each of the following rate equation:

Rate $= k [{BrO}_{3}^{-}] [{Br}^{-}] {[H^{+}]}^{2}$

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 3

State the units of $k$ corresponding to each of the following rate equation:

Rate $= k [cyclopropane]$

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 4

Draw sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction:

$NO (g) + CO (g) + O_{2} (g) \to {NO}_{2} (g) + {CO}_{2} (g)$ for which the rate equation is: rate $= k {[NO]}^{2}$

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 4

Draw sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction:

$2 HI (g) \overset{gold}{\to} H_{2} (g) + I_{2} (g)$ for which the rate equation is: $rate = k$

Note: the catalyst influences the order here – the order is not the same as for the uncatalysed reaction

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 4

Draw sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction:

${({CH}_{3})}_{3} CCl + {OH}^{-} \to {({CH}_{3})}_{3} COH + {Cl}^{-}$ for which the rate equation is: $k [{({CH}_{3})}_{3} CCl]$

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 5

Draw a sketch graph to show how the concentration of the bold reactant changes with time.

$NO (g) + CO (g) + O_{2} (g) \to {NO}_{2} (g) + {CO}_{2} (g)$ for which the rate equation is: rate $= k {[NO]}^{2}$

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 5

Draw a sketch graph to show how the concentration of the bold reactant changes with time.

$2 HI (g) \overset{gold}{\to} H_{2} (g) + I_{2} (g)$ for which the rate equation is: $rate = k$

Note: the catalyst influences the order here – the order is not the same as for the uncatalysed reaction

State the units of k corresponding to each of the following rate equation: Rate = k[NO]2

Important Questions on Reaction Kinetics

Learn and Prepare for any exam you want !

State the units of $k$ corresponding to each of the following rate equation:

Rate $= k {[NO]}^{2}$