# CBSE Class 12-science Chemistry Integrated Rate Equation

Study better with TopperLearning’s CBSE Class 12 Science Chemistry Chemical Kinetics – Integrated Rate Equation learning resources such as practice tests, NCERT solutions etc. Learn to derive the integrated rate equation with the step-wise explanation provided by an experienced Chemistry expert in our concept videos. Our topic notes for Chemistry will enable you to have a quick look at key concepts related to the integrated rate equation.

Practise our CBSE Class 12 Science Chemistry textbook solutions to learn to use the half-life formula for the calculations involving the first-order, second-order or zero-order reactions. To make sure that you remember the problem-solving methods in your board exam, take mock exams using our sample papers and previous years’ Chemistry papers.

## Videos

- Please ans both part
- Explain why the rate of a chemical reaction does not remain uniform throughout the reaction?
- For a chemical reaction X Y, The rate increases by the factor 2.25 when concentration of X is increased by 1.5. Derive or suggest the rate law equation and find the order of reaction.
- A gas phase decomposition of xy follows the rate law r = k[xy]
^{n}. what are the units of its rate constant? - The reaction A + 3B 2C obeys the rate equation: Rate = k[A]
^{1/3}[B]^{3/2}. Find out the order of this reaction? - The experimental data for the reaction:
2A + B
_{2}→ 2AB is: Write the rate equation for the reaction? - The half-life of a first order decomposition of nitramide is 2.1 hour at 25
^{o}C. Determine the time taken for the compound to decompose 99% of its original amount, rate constant = 0.2303 per hour. - The rate of reaction between A and B increases by a factor of 100. Calculate the order of the reaction when the concentration of A is increased 10 times.
- Calculate the rate of reaction from the rate law:
_{}= k[A] [B]^{2}, when the concentration of A and B are 0.01 M and 0.02 M respectively and k = 5.1 x 10^{-3}L^{2}mol^{-2}s^{-1}. - Derive an equation for calculating the half life of a first order reaction

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