Advertisements
Advertisements
Question
Derive integrated rate law for zero order reaction.
Advertisements
Solution
Consider a zero-order reaction, \[\ce{A -> Product}\]
The rate of the reaction is:
Rate = `-(d[A])/dt`
By the rate law,
Rate = k × [A]0 = k
On rearranging the equation,
∴ d[A] = k × dt
If [A]0 is the initial concentration of the reactant A at t = 0 and [A]t is the concentration of A present after time t, then by integrating the above equation,
`int_([A]_0)^([A]_t) - d[A] = int_(t = 0)^(t = t) k dt`
`- int_([A]_0)^([A]_t) d [A] = kint_(0)^(t) dt`
`[A]_([A]_0)^([A]_t) = k [t]_0^t`
−([A]t − [A]0) = kt
∴ [A]0 − [A]t = kt
∴ k = `([A]_0 - [A]_t)/t`
RELATED QUESTIONS
The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production of N2 and H2 if k = 2.5 × 10−4 mol−1 L s−1?
The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
| Experiment | A/mol L−1 | B/mol L−1 | Initial rate/mol L−1 min−1 |
| I | 0.1 | 0.1 | 2.0 × 10−2 |
| II | ______ | 0.2 | 4.0 × 10−2 |
| III | 0.4 | 0.4 | ______ |
| IV | ______ | 0.2 | 2.0 × 10−2 |
The decomposition of NH3 on a platinum surface is a zero-order reaction. If the rate constant (k) is 4 x 10-3 ms-1, how long will it take to reduce the initial concentration of NH3 from 0.1 M to 0.064 M?
Give one example of zero order reaction.
Derive integrated rate law for a zero-order reaction \[\ce{A -> Product}\].
Which of the following graphs is correct for a zero order reaction?
Write the rate equation for the reaction `2A + B -> C` if the order of the reaction is zero.
Derive an expression to calculate time required for completion of zero order reaction.
For a zero order reaction will the molecularity be equal to zero? Explain.
Consider the following statement:-
(i) Increase in concentration of reactant increases the rate of a zero-order reaction.
(ii) Rate constant k is equal to collision frequency A if Ea = 0
(iii) Rate constant k is equal to collision frequency A if Ea = 0
(iv) In k vs t is a straight line
(v) In k vs 1/T is a straight line
Which of the above statement is correct?
Write the expression of integrated rate equation for zero order reaction.
The slope in the plot of [R] Vs. time for a zero-order reaction is ______.
The following experimental rate data were obtained for a reaction carried out at 25°C:
\[\ce{A_{(g)} + B_{(g)} -> C_{(g)} + A_{(g)}}\]
| Initial [A(g)]/mol dm−3 | Initial [B(g)]/mol dm−3 | Initial rate/mol dm−3s−1 |
| 3.0 × 10−2 | 2.0 × 10−2 | 1.89 × 10−4 |
| 3.0 × 10−2 | 4.0 × 10−2 | 1.89 × 10−4 |
| 6.0 × 10−2 | 4.0 × 10−2 | 7.56 × 10−4 |
What are the orders with respect to A(g) and B(g)?
Assertion (A): For a zero-order reaction, the unit of rate constant and rate of reaction are same.
Reason (R): Rate of reaction for zero order reaction is independent of concentration of reactant.
If the initial concentration of substance A is 1.5 M and after 120 seconds the concentration of substance A is 0.75 M, the rate constant for the reaction if it follows zero-order kinetics is ______.
What is zeroth order reaction? Derive its integrated rate Law. What are the units of rate constant?
Write the unit of rate constant of zero order reaction.
What is zero order reaction?
If unit of rate constant is mol dm−3s−1, the order of reaction would be ______.
