Advertisements
Advertisements
Question
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?
Advertisements
Solution
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
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?
Derive integrated rate law for a zero-order reaction \[\ce{A -> Product}\].
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?
For a zero-order reaction, the plot of [A]t vs t is linear with a ______
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)?
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?
