Advertisements
Advertisements
प्रश्न
In a reaction between A and B, the initial rate of reaction (r0) was measured for different initial concentrations of A and B as given below:
| A/mol L−1 | 0.20 | 0.20 | 0.40 |
| B/mol L−1 | 0.30 | 0.10 | 0.05 |
| r0/mol L−1 s−1 | 5.07 × 10−5 | 5.07 × 10−5 | 1.43 × 10−4 |
What is the order of the reaction with respect to A and B?
उत्तर
`"dx"/"dt"` = k[A]x [B]y
5.07 × 10−5 = k(0.2)x (0.3)y ...(i)
5.07 × 10−5 = k(0.2)x (0.10)y ...(ii)
Dividing (i) by (ii), we get
1 = 3y ⇒ 30
3y ⇒ y = 0
5.07 × 10−5 = k(0.2)x (0.1)0 ...(iii)
1.43 × 10−4 = k(0.4)x (0.05)0 ...(iv)
Dividing (iv) by (iii), we get 2.8 = 2x
log 2.8 = x log 2
or x = `log2.8/log2.0`
= `0.4472/0.3010`
= 1.48
≈ 1.5
The order of reaction is 1.5 with respect to 'A' and zero with respect to 'B'.
APPEARS IN
संबंधित प्रश्न
In a first order reaction x → y, 40% of the given sample of compound remains unreacted in 45 minutes. Calculate rate constant of the reaction.
What is pseudo first order reaction? Give one· example of it.
For a reaction A + B ⟶ P, the rate is given by
Rate = k [A] [B]2
How is the rate of reaction affected if the concentration of B is doubled?
From the rate expression for the following reaction, determine the order of reaction and the dimension of the rate constant.
\[\ce{CH3CHO_{(g)} -> CH4_{(g)} + CO_{(g)}}\] Rate = k [CH3CHO]3/2
For the reaction: \[\ce{2A + B → A2B}\] the rate = k[A][B]2 with k = 2.0 × 10−6 mol−2 L2 s−1. Calculate the initial rate of the reaction when [A] = 0.1 mol L−1, [B] = 0.2 mol L−1. Calculate the rate of reaction after [A] is reduced to 0.06 mol L−1.
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?
Define the following terms:
Pseudo first-order reaction
Which of the following statement is true for order of a 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 ______.
In a reaction if the concentration of reactant A is tripled, the rate of reaction becomes twenty seven times. What is the order of the reaction?
Why can’t molecularity of any reaction be equal to zero?
In the presence of a catalyst, the heat evolved or absorbed during the reaction.
For a reaction A + B → products, the rate law is given by: r = `K[A]^(1/2)`. What is the order of reaction?
For a reaction R → p the concentration of reactant change from 0.03 m to 0.02 m in minute, calculate the average rate of the reaction using the unit of second.
For a reaction \[\ce{Cl2l(g) + 2No(g) -> 2NaCl(g)}\] the rate law is expressed as rate= K[Cl2] [No]2 what is the order of the reaction?
The rate of a chemical reaction double for every 10° rise in temperature. If the temperature is raised. by 50°C, the rate of relation by about:-
At concentration of 0.1 and 0.2 mol L–1 the rates of deem position of a compound were found to be 0.18 and 0.72 mol L–1 m–1. What is the order of the reaction?
