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प्रश्न
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?
उत्तर
Given that:
k = 4 x 10-3 Ms-1
`["A"_°]` = 0.1 M
[A] = 0.064 M
For a zero-order reaction,
k=`1/t {["A"_°]-["A"]}`
4 x 10-3 Ms-1 = `1/"t" {[0.1]-[0.064]}`
t =`( 0.1-0.064)/(4xx10^-3)=0.009xx10^3=9` seconds
संबंधित प्रश्न
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 |
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.
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.
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Derive the expression for integrated rate law for zero order reaction A → Products.
Write the unit of rate constant of zero order reaction.
If unit of rate constant is mol dm−3s−1, the order of reaction would be ______.
