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Decomposition of h2o2 follows a first order reaction. In fifty minutes the concentration of h2o2 decreases from 0.5 to 0.125 M in one such decomposition . When the concentration of h2o2 reaches 0.05 M, the rate of formation of O2 will be :- And :- 6.93 • 10' -4( ten raised to power -4) how?
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Decomposition of h2o2 follows a first order reaction. In fifty minutes...
2H2O2 → 2H2O + O2
In 50 minutes, the concentration is reduced to one fourth
(∵ 0.5/0.125 = 4)
Hence 2 half life periods correxponds to 50 minutes.
t(1/2) ​= 25 min
The rate constant k = 0.693/t(1/2)
= 0.693/25 
Rate of decomposition of H2 x O2 ​= k[H2O2] = 0.693/25 x 0.05 = 1.39 x 10^−3 mol/min
Rate of formation of oxygen is one half the rate of decomposition of H2O2​ .
It is 1/2 x 1.39 x 10^−3 = 6.93 x 10^−4 mol/min
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Decomposition of h2o2 follows a first order reaction. In fifty minutes...
Decomposition of H2O2

Introduction: H2O2 is a chemical compound that decomposes into water and oxygen. This decomposition reaction occurs at different rates depending on various factors such as temperature and concentration of the reactants.

First-Order Reaction: The decomposition of H2O2 follows a first-order reaction, which means that the rate of reaction is directly proportional to the concentration of the reactant.

Given Data: In fifty minutes, the concentration of H2O2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be calculated.

Calculations:

- To determine the rate constant of the reaction, we can use the formula for first-order reaction: k = (-1/t) x ln([H2O2]t/[H2O2]0), where t is the time, [H2O2]t is the concentration of H2O2 at time t, [H2O2]0 is the initial concentration of H2O2, and ln is the natural logarithm.
- Using the given data, we can calculate the rate constant k: k = (-1/50) x ln(0.125/0.5) = 0.0280 min^-1.
- When the concentration of H2O2 reaches 0.05 M, we can use the first-order rate equation to calculate the rate of formation of O2: rate = k[H2O2] = 0.0280 x 0.05 = 6.93 x 10^-4 M/min.

Conclusion: When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be 6.93 x 10^-4 M/min.
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Read the passage given below and answer the following questions:The rate of a reaction, which may also be called its velocity or speed, can be defined with relation to the concentration of any of the reacting substances, or to that of any product of the reaction. If the species chosen is a reactant which has a concentration c at time t the rate is - dc/dt, while the rate with reference to a product having a concentration x at time t is dx/dt. Any concentration units may be used for expressing the rate; thus, if moles per liter are employed for concentration and seconds for the time, the units for the rate are moles litre–1sec–1. For gas reactions pressure units are sometimes used in place of concentrations, so that legitimate units for the rate would be (mm. Hg) sec–1 and atm. sec–1 The order of a reaction concerns the dependence of the rate upon the concentrations of reacting substances; thus, if the rate is found experimentally to be proportional to the ath power of the concentration of one of the reactants A, to the both power of the concentration of a second reactant B, and so forth, via., rate = k CAα CAβ the over-all order of the reaction is simply n = α + β + ----- (2) Such a reaction is said to be of the αth order with respect to the substance A, the βth order with respect to B.In the following questions, a statement of Assertion followed by a statement of Reason is given. Choose the correct answer out of the following choices on the basis of the above passage.Assertion: Rate of reaction is a measure of change in concentration of reactant with respect to time.Reason: Rate of reaction is a measure of change in concentration of product with respect to time.

Read the passage given below and answer the following questions:The rate of a reaction, which may also be called its velocity or speed, can be defined with relation to the concentration of any of the reacting substances, or to that of any product of the reaction. If the species chosen is a reactant which has a concentration c at time t the rate is - dc/dt, while the rate with reference to a product having a concentration x at time t is dx/dt. Any concentration units may be used for expressing the rate; thus, if moles per liter are employed for concentration and seconds for the time, the units for the rate are moles litre–1sec–1. For gas reactions pressure units are sometimes used in place of concentrations, so that legitimate units for the rate would be (mm. Hg) sec–1 and atm. sec–1 The order of a reaction concerns the dependence of the rate upon the concentrations of reacting substances; thus, if the rate is found experimentally to be proportional to the ath power of the concentration of one of the reactants A, to the both power of the concentration of a second reactant B, and so forth, via., rate = k CAα CAβ the over-all order of the reaction is simply n = α + β + ----- (2) Such a reaction is said to be of the αth order with respect to the substance A, the βth order with respect to B.In the following questions, a statement of Assertion followed by a statement of Reason is given. Choose the correct answer out of the following choices on the basis of the above passage.Assertion: The unit of k is independent of order of reaction.Reason: The unit of k is moles L–1s–1.

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Decomposition of h2o2 follows a first order reaction. In fifty minutes the concentration of h2o2 decreases from 0.5 to 0.125 M in one such decomposition . When the concentration of h2o2 reaches 0.05 M, the rate of formation of O2 will be :- And :- 6.93 • 10' -4( ten raised to power -4) how?
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Decomposition of h2o2 follows a first order reaction. In fifty minutes the concentration of h2o2 decreases from 0.5 to 0.125 M in one such decomposition . When the concentration of h2o2 reaches 0.05 M, the rate of formation of O2 will be :- And :- 6.93 • 10' -4( ten raised to power -4) how? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Decomposition of h2o2 follows a first order reaction. In fifty minutes the concentration of h2o2 decreases from 0.5 to 0.125 M in one such decomposition . When the concentration of h2o2 reaches 0.05 M, the rate of formation of O2 will be :- And :- 6.93 • 10' -4( ten raised to power -4) how? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Decomposition of h2o2 follows a first order reaction. In fifty minutes the concentration of h2o2 decreases from 0.5 to 0.125 M in one such decomposition . When the concentration of h2o2 reaches 0.05 M, the rate of formation of O2 will be :- And :- 6.93 • 10' -4( ten raised to power -4) how?.
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