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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:
  • a)
    2.66 L min–1 at STP
  • b)
    1.34 × 10–2 mol min–1
  • c)
    6.96 × 10–2 mol min–1
  • d)
    6.93 × 10–4 mol min–1
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
Decomposition of H2O2 follows a first order reaction. In fifty minute...
For a first order reaction
Given a = 0.5 , (a - x) = 0.125, t = 50 min
∴
= 2.78 x 10-2min-1
r = k[H2O2] = 2.78 x 10-2 x 0.05
= 1.386 x 10-3 mol min-1
Now,
=
= 6.93 x 10-4 mol min-1
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Decomposition of H2O2 follows a first order reaction. In fifty minute...
Decomposition of H2O2

The decomposition of hydrogen peroxide (H2O2) follows a first-order reaction. This means that the rate of decomposition is directly proportional to the concentration of H2O2.


Given Information

In fifty minutes, the concentration of H2O2 decreases from 0.5 to 0.125 M.


Calculating the Rate Constant

Since the reaction follows a first-order kinetics, we can use the integrated rate equation:

ln([A]t/[A]0) = -kt

Where [A]t is the concentration at time t, [A]0 is the initial concentration, k is the rate constant, and t is the time.


Using the given information, we can substitute the values into the equation:

ln(0.125/0.5) = -k(50)

Simplifying the equation gives:

-1.09861 = -50k

Solving for k:

k = 0.0219722 min^-1


Calculating the Rate of Formation of O2

The rate of formation of O2 is equal to half the rate of decomposition of H2O2, as the balanced chemical equation for the decomposition of H2O2 is:

2H2O2 -> 2H2O + O2


At the point when the concentration of H2O2 reaches 0.05 M, we can calculate the rate of formation of O2 using the rate constant (k) we obtained earlier.

Using the first-order rate equation:

k = ln([A]0/[A]t)

Substituting the values:

0.0219722 = ln(0.5/0.05)

Simplifying the equation gives:

0.0219722 = ln(10)

Taking the anti-logarithm of both sides:

10^(0.0219722) = 1.051


Multiplying this value by 2 (as the rate of formation of O2 is half the rate of decomposition of H2O2) gives:

2 * 1.051 = 2.102


Therefore, the rate of formation of O2 when the concentration of H2O2 reaches 0.05 M is approximately 2.102 L min^-1 at STP. This corresponds to option 'D': 6.93 × 10^(-4) mol min^(-1).
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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: The unit of k is independent of order of reaction.Reason: The unit of k is moles L–1s–1.

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.

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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:a)2.66 L min–1 at STPb)1.34 × 10–2 mol min–1c)6.96 × 10–2 mol min–1 d)6.93 × 10–4 mol min–1Correct answer is option 'D'. Can you explain this answer?
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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:a)2.66 L min–1 at STPb)1.34 × 10–2 mol min–1c)6.96 × 10–2 mol min–1 d)6.93 × 10–4 mol min–1Correct answer is option 'D'. Can you explain this answer? 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:a)2.66 L min–1 at STPb)1.34 × 10–2 mol min–1c)6.96 × 10–2 mol min–1 d)6.93 × 10–4 mol min–1Correct answer is option 'D'. Can you explain this answer? 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:a)2.66 L min–1 at STPb)1.34 × 10–2 mol min–1c)6.96 × 10–2 mol min–1 d)6.93 × 10–4 mol min–1Correct answer is option 'D'. Can you explain this answer?.
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