Advertisements
Advertisements
Question
The following data were obtained during the first order thermal decomposition of SO2Cl2 at a constant volume :
SO2Cl2 (g) → SO2 (g) + Cl2 (g)
| Experiment | Time/s–1 | Total pressure/atm |
| 1 | 0 | 0.4 |
| 2 | 100 | 0.7 |
Calculate the rate constant.
(Given : log 4 = 0.6021, log 2 = 0.3010)
Advertisements
Solution 1
The given reaction is as follows:
SO2Cl2 (g) → SO2(g)+Cl2(g)
Also given:
| Experiment | Time/s–1 | Total pressure/atm |
| 1 | 0 | 0.4 |
| 2 | 100 | 0.7 |
The rate constant k can be calculated as follows:
`k=2.303/tlog `
when t= 100s, k = `2.303/(100s)log`
`k = 2.303/(100s)log`
`k=2.303/(100s) log 4`
`k = 2.303/(100s)xx0.6021`
k = 1.39 x 10-2s-1
Therefore, the rate constant is 1.39 x 10-2s-1
Solution 2
The thermal decomposition of SO2Cl2 at a constant volume is represented by the following equation:
SO2Cl2→SO2(g) + Cl2(g)
At t =0 P0 0 0
At t=t P0 −p p p
After time t, total pressure is given as:
Pt =(P0−p) + p + p
Pt = P0 + p
This, on rearrangement, gives:
p = Pt − P0
∴ P0−p=P0−(Pt−P0)= 2P0 − Pt
For the first-order reaction, we have:
`k=2.303/tlog P_0/(P_0 - p)`
`=2.303/tlog P_0/(P_0 - p)`
t = 100 s
`k = 2.303/100log 0.42/(0.4 - 0.7) = 1.386 xx 10^(-2)s-1`
APPEARS IN
RELATED QUESTIONS
From the rate expression for the following reaction, determine the order of reaction and the dimension of the rate constant.
\[\ce{C2H5Cl_{(g)} -> C2H4_{(g)} + HCl_{(g)}}\] Rate = k[C2H5Cl]
Mention the factors that affect the rate of a chemical reaction.
A reaction is first order in A and second order in B. How is the rate affected on increasing the concentration of B three times?
For a reaction R ---> P, half-life (t1/2) is observed to be independent of the initial concentration of reactants. What is the order of reaction?
Consider a first order gas phase decomposition reaction given below :
\[\ce{A(g) -> B(g) + C(g)}\]
The initial pressure of the system before decomposition of A was pi. After lapse of time ‘t’, total pressure of the system increased by x units and became ‘pt’ The rate constant k for the reaction is given as ______.
Which of the following statements is not correct about order of a reaction.
For which type of reactions, order and molecularity have the same value?
The rate constant for the reaction \[\ce{2H2O5 -> 4NO2 + O2}\] is 30 × 10–5 sec–1. if the rate is 204 × 10–5 mol L–1 S–1, then the concentration of N2O5 (in mol–1) is-
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is reduced to half?
Higher yield of NO in \[\ce{N2(g) + O2 <=> 2NO(g)}\] can be obtained at:
[ΔH of the reaction = +180.7 kJ mol−1]
- higher temperature
- lower temperature
- higher concentration of N2
- higher concentration of O2
Choose the correct answer from the options given below:
