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The variation of concentration of 'A' with time in two experiments starting with two different initial concentration of 'A' is given by the following graph. The reaction is represented by A (aq.) B (aq.) what is rate of reaction (M/min.) when conc. of A in aqueous solution was 1.8M:?
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?The variation of concentration of 'A' with time in two experiments st...
During first five minutes, the concentration decreases from 1.5  M to  1.2  M.
Thus, the rate of the reaction is  
During next 5 minutes, the concentration decreases from 1.2 M to 1.0 M
The rate of the reaction is  

The reaction is of the first order
The rate law expression is 
The rate constant is k= 1/25
​
Hence, the rate when the concentration is  1.8 M is r 
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?The variation of concentration of 'A' with time in two experiments st...
Understanding the Rate of Reaction
The rate of a chemical reaction is typically defined as the change in concentration of a reactant or product per unit time. In this case, we are focusing on the concentration of A as it changes over time.
Concentration of A
- The concentration of A decreases as the reaction proceeds.
- To determine the rate of reaction when the concentration of A is 1.8 M, we need to analyze the graph provided.
Rate Calculation
- Identify the time interval during which the concentration of A changes from its initial value to 1.8 M.
- Measure the change in concentration (Δ[A]) and the corresponding time interval (Δt) from the graph.
- The rate of reaction can be calculated using the formula: Rate = Δ[A] / Δt.
Example Calculation
- If, for instance, the concentration of A decreases from 2.0 M to 1.8 M over a time period of 2 minutes:
- Δ[A] = 1.8 M - 2.0 M = -0.2 M
- Δt = 2 minutes
- Plugging these values into the formula:
- Rate = -0.2 M / 2 min = -0.1 M/min
Interpreting the Rate
- The negative sign indicates that the concentration of A is decreasing.
- The absolute value of the rate (0.1 M/min) represents the speed of the reaction at the specified concentration.
Conclusion
- By examining the graph and applying the rate calculation method, you can determine the rate of reaction for any concentration of A, including when it is 1.8 M.
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Not all chemical reactions proceed to a stage at which the concentrations of the reactants become vanishingly small. Here we consider the kinetics of such reactions.Let a reaction be represented in general terms by the schemewhere k., and k_., represent the rate constants for the forwards and reverse reactions, respectively. The equilibrium constant for this reaction may be written asK = [B] /[A] = K1/K1 --(1)where the subscript 00 refers to a time t, sufficiently long to establish equilibrium at the given temperature. The initial concentration of species A is [A]O, and that of B is [B]O . After a time t, let the concentration of species A be [A/t and that of B be [Bat. The total rate of change of [At is given byd[A]t/dt= - K1[A]t + k-1[B]tIf, as is usual, [B]O is initially zero, it follows from a mass balance that at any time t,[Bat = [A]0 - [A]t, whenced[A]t/dt = K1[A]t + k-1([A]O - [A]t)ord[A]t/dt = (K1 + k-1)For the reaction (having both 1ts order reactions), the concentration as a function of time are given for a certain experimental run along with a tangent to the graph at the origin. The ratio of the magnitude of the slopes of the graph of [A/ and [C/ at the origin would be

Not all chemical reactions proceed to a stage at which the concentrations of the reactants become vanishingly small. Here we consider the kinetics of such reactions.Let a reaction be represented in general terms by the schemewhere k., and k_., represent the rate constants for the forwards and reverse reactions, respectively. The equilibrium constant for this reaction may be written asK = [B] /[A] = K1/K1 --(1)where the subscript 00 refers to a time t, sufficiently long to establish equilibrium at the given temperature. The initial concentration of species A is [A]O, and that of B is [B]O . After a time t, let the concentration of species A be [A/t and that of B be [Bat. The total rate of change of [At is given byd[A]t/dt= - K1[A]t + k-1[B]tIf, as is usual, [B]O is initially zero, it follows from a mass balance that at any time t,[Bat = [A]0 - [A]t, whenced[A]t/dt = K1[A]t + k-1([A]O - [A]t)ord[A]t/dt = (K1 + k-1)At what time is the rate of change of concentration of A equal to rate of change of concentration of C in magnitude ?

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?The variation of concentration of 'A' with time in two experiments starting with two different initial concentration of 'A' is given by the following graph. The reaction is represented by A (aq.) B (aq.) what is rate of reaction (M/min.) when conc. of A in aqueous solution was 1.8M:?
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?The variation of concentration of 'A' with time in two experiments starting with two different initial concentration of 'A' is given by the following graph. The reaction is represented by A (aq.) B (aq.) what is rate of reaction (M/min.) when conc. of A in aqueous solution was 1.8M:? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about ?The variation of concentration of 'A' with time in two experiments starting with two different initial concentration of 'A' is given by the following graph. The reaction is represented by A (aq.) B (aq.) what is rate of reaction (M/min.) when conc. of A in aqueous solution was 1.8M:? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for ?The variation of concentration of 'A' with time in two experiments starting with two different initial concentration of 'A' is given by the following graph. The reaction is represented by A (aq.) B (aq.) what is rate of reaction (M/min.) when conc. of A in aqueous solution was 1.8M:?.
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