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Zero Order Reactions

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Questions on zero order reactions - example

Zero Order Kinetics - definition

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Class 12 Medical - Integrated Rate Equations Class 12 Engineering - Integrated Rate Equations

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Integrated Rate Law Equation for Zero Order Reaction

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Plot the graph between Concentration, Rate and Time for Zero Order Reactions

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Numericals on zero order reactions

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Integrated Rate Law Equation for Zero Order Reaction

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The rate constant for disappearance of reactant as mentioned in is $2 \times 1 0^{- 2} m o l L^{- 1} s e c^{- 1}$ , if the concentration of the reactant after 25 sec is 0.25M, the initial concentration is:

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The unit of rate constant for zero order reaction is:

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The time for the half-life period of a certain reaction $A \to$ products is $1$ hour. When the initial concentration of the reactant, $A$ is $2.0 m o l L^{- 1}$ . How much time does it take initial concentration to make from $0.50$ to $0.25 m o l L^{- 1}$ if it is a zero-order reaction?

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Which of the following graphs are correct for a zero - order reaction?

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K for a zero order reaction is $2 \times 10^{- 2} L^{- 1} S e c^{- 1}$ . If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been.

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Which of the following curves represent(s) a zero-order reaction ?

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In a zero-order reaction:

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Which of the following graphs is correct for the following reaction?
$C H_{3} - C H_{2} - C H = C H_{2} H_{2} / N i 300^{o} C C H_{3} - C H_{2} - C H_{2} - C H_{3}$

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Which of the following curves represents a zero order reaction?

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K for a zero order reaction is $2 \times 1 0^{- 2} m o l L^{- 1} s e c^{- 1}$ . If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been:

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Questions on zero order reactions - example

Zero Order Kinetics - definition

Also available in

Related Concepts

First Order Reaction

Half Life of a Reaction

Pseudo First Order Reaction

Learn with Videos

Quick summary with Stories

Integrated Rate Law Equation for Zero Order Reaction

Related questions

The rate constant for disappearance of reactant as mentioned in is 2×10−2molL−1sec−1, if the concentration of the reactant after 25 sec is 0.25M, the initial concentration is:

The unit of rate constant for zero order reaction is:

The time for the half-life period of a certain reaction A→ products is 1 hour. When the initial concentration of the reactant, A is 2.0 mol L−1. How much time does it take initial concentration to make from 0.50 to 0.25 mol L−1 if it is a zero-order reaction?

Which of the following graphs are correct for a zero - order reaction?

K for a zero order reaction is 2×10−2L−1Sec−1. If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been.

Which of the following curves represent(s) a zero-order reaction ?

In a zero-order reaction:

Which of the following graphs is correct for the following reaction? CH3​−CH2​−CH=CH2​H2​/Ni300oC​CH3​−CH2​−CH2​−CH3​

Which of the following curves represents a zero order reaction?

K for a zero order reaction is 2×10−2molL−1sec−1. If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been:

The rate constant for disappearance of reactant as mentioned in is $2 \times 1 0^{- 2} m o l L^{- 1} s e c^{- 1}$ , if the concentration of the reactant after 25 sec is 0.25M, the initial concentration is:

The time for the half-life period of a certain reaction $A \to$ products is $1$ hour. When the initial concentration of the reactant, $A$ is $2.0 m o l L^{- 1}$ . How much time does it take initial concentration to make from $0.50$ to $0.25 m o l L^{- 1}$ if it is a zero-order reaction?

K for a zero order reaction is $2 \times 10^{- 2} L^{- 1} S e c^{- 1}$ . If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been.

Which of the following graphs is correct for the following reaction?
$C H_{3} - C H_{2} - C H = C H_{2} H_{2} / N i 300^{o} C C H_{3} - C H_{2} - C H_{2} - C H_{3}$

K for a zero order reaction is $2 \times 1 0^{- 2} m o l L^{- 1} s e c^{- 1}$ . If the concentration of the reactant after 25 sec is 0.5 M, the initial concentration must have been: