Advertisements
Advertisements
प्रश्न
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 ______.
पर्याय
`k = 2.303/t log p_i/(p_i - x)`
`k = 2.303/t log p_i/(2p_i - p_t)`
`k = 2.303/t log p_i/(2p_i + p_t)`
`k = 2.303/t log p_i/(p_i + x)`
Advertisements
उत्तर
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 `k = 2.303/t log p_i/(2p_i - p_t)`.
Explanation:
Consider a first order gas phase decomposition reaction:
\[\ce{A_{(g)} -> B_{(g)} + C_{(g)}}\]
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'.
In other words, the pressure of A decreased by x atom.
\[\ce{A_{(g)} -> B_{(g)} + C_{(g)}}\]
Initial pressure: Pi atm
Pressure after time t: (Pi – x) atm x atm x atm
Pt = (Pi – x) + x + x = Pi + x atm
x = Pt – Pi
PA = Pressure of A after time t = Pi - x = Pi - (Pi - Pi) = 2Pi - Pt
`k = 2.303/t log (["A"]_0)/(["A"])`
= `k = 2.303/t log p_i/(2p_i - p_t)`
APPEARS IN
संबंधित प्रश्न
A reaction is second order in A and first order in B.
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of A three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
Write two factors that affect the rate of reaction.
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?
For the hydrolysis of methyl acetate in aqueous solution, the following results were obtained :
| t/s | 0 | 30 | 60 |
| [CH3COOCH3] / mol L–1 | 0.60 | 0.30 | 0.15 |
(i) Show that it follows pseudo first order reaction, as the concentration of water remains constant.
(ii) Calculate the average rate of reaction between the time interval 30 to 60 seconds.
(Given log 2 = 0.3010, log 4 = 0.6021)
For a reaction, \[\ce{A + B -> Product}\]; the rate law is given by, r = k [A]1/2 [B]2. What is the order of the reaction?
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is doubled?
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?
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?
Write resonating structures of ozone.
Rate of reaction for the combustion of propane is equal to:
\[\ce{C3H8_{(g)} + 5O2_{(g)} -> 3CO2_{(g)} + 4H2O_{(g)}}\]
Which of the following statement is true for order of a reaction?
Consider the reaction A ⇌ B. The concentration of both the reactants and the products varies exponentially with time. Which of the following figures correctly describes the change in concentration of reactants and products with time?
Why does the rate of any reaction generally decreases during the course of the reaction?
Why can’t molecularity of any reaction be equal to zero?
Assertion: Rate constants determined from Arrhenius equation are fairly accurate for simple as well as complex molecules.
Reason: Reactant molecules undergo chemical change irrespective of their orientation during collision.
Use Molecular Orbital theory to determine the bond order in each of species, [He2j+ and [He2]2+?
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 first order A → B, the reaction rate at reactant concentration of 0.01 m is found to be 2.0 × 10–5. The half-life period of reaction.
Identify the order of reaction from the following unit for its rate constant:
L mol–1 s–1
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:
