To determine which of the given options is correctly matched at constant temperature, we need to analyze each option one by one:

(1) t × a = constant, for 2nd order kinetics:
For a 2nd order reaction, the rate equation is given by rate = k × [A]^2, where [A] represents the concentration of reactant A.
Integrating this rate equation gives us the equation t = 1 / (k × [A]₀), where [A]₀ is the initial concentration of reactant A.
From this equation, we can see that t × a is not constant for 2nd order kinetics. Therefore, option (1) is incorrect.

(2) t × a = constant, for 1st order kinetics:
For a 1st order reaction, the rate equation is given by rate = k × [A], where [A] represents the concentration of reactant A.
Integrating this rate equation gives us the equation t = ln([A]₀ / [A]) / k, where [A]₀ is the initial concentration of reactant A.
From this equation, we can see that t × a is not constant for 1st order kinetics. Therefore, option (2) is incorrect.

(3) t × a = constant, for zero order kinetics:
For a zero order reaction, the rate equation is given by rate = k.
Integrating this rate equation gives us the equation [A] = [A]₀ - k × t, where [A] represents the concentration of reactant A.
From this equation, we can see that t × a is constant for zero order kinetics. Therefore, option (3) is correct.

(4) Unit of rate constant is M sec for 1st order:
The unit of rate constant depends on the overall order of the reaction. For a 1st order reaction, the unit of rate constant is sec⁻¹. Therefore, option (4) is incorrect.

In conclusion, the correct option is (3) t × a = constant, for zero order kinetics.

Question

To determine which of the given options is correctly matched at constant temperature, we need to analyze each option one by one:

(1) t × a = constant, for 2nd order kinetics:
For a 2nd order reaction, the rate equation is given by rate = k × [A]^2, where [A] represents the concentration of reactant A. 
Integrating this rate equation gives us the equation t = 1 / (k × [A]₀), where [A]₀ is the initial concentration of reactant A.
From this equation, we can see that t × a is not constant for 2nd order kinetics. Therefore, option (1) is incorrect.

(2) t × a = constant, for 1st order kinetics:
For a 1st order reaction, the rate equation is given by rate = k × [A], where [A] represents the concentration of reactant A.
Integrating this rate equation gives us the equation t = ln([A]₀ / [A]) / k, where [A]₀ is the initial concentration of reactant A.
From this equation, we can see that t × a is not constant for 1st order kinetics. Therefore, option (2) is incorrect.

(3) t × a = constant, for zero order kinetics:
For a zero order reaction, the rate equation is given by rate = k.
Integrating this rate equation gives us the equation [A] = [A]₀ - k × t, where [A] represents the concentration of reactant A.
From this equation, we can see that t × a is constant for zero order kinetics. Therefore, option (3) is correct.

(4) Unit of rate constant is M sec for 1st order:
The unit of rate constant depends on the overall order of the reaction. For a 1st order reaction, the unit of rate constant is sec⁻¹. Therefore, option (4) is incorrect.

In conclusion, the correct option is (3) t × a = constant, for zero order kinetics.

Knowee AI · Accepted Answer

To determine which of the given options is correctly matched at constant temperature, we need to analyze each option one by one:

(1) t × a = constant, for 2nd order kinetics:
For a 2nd order reaction, the rate equation is given by rate = k × [A]^2, where [A] represents the concentration of reactant A. 
Integrating this rate equation gives us the equation t = 1 / (k × [A]₀), where [A]₀ is the initial concentration of reactant A.
From this equation, we can see that t × a is not constant for 2nd order kinetics. Therefore, option (1) is incorrect.

(2) t × a = constant, for 1st order kinetics:
For a 1st order reaction, the rate equation is given by rate = k × [A], where [A] represents the concentration of reactant A.
Integrating this rate equation gives us the equation t = ln([A]₀ / [A]) / k, where [A]₀ is the initial concentration of reactant A.
From this equation, we can see that t × a is not constant for 1st order kinetics. Therefore, option (2) is incorrect.

(3) t × a = constant, for zero order kinetics:
For a zero order reaction, the rate equation is given by rate = k.
Integrating this rate equation gives us the equation [A] = [A]₀ - k × t, where [A] represents the concentration of reactant A.
From this equation, we can see that t × a is constant for zero order kinetics. Therefore, option (3) is correct.

(4) Unit of rate constant is M sec for 1st order:
The unit of rate constant depends on the overall order of the reaction. For a 1st order reaction, the unit of rate constant is sec⁻¹. Therefore, option (4) is incorrect.

In conclusion, the correct option is (3) t × a = constant, for zero order kinetics.

Which of the following is correctly matched(at constant temperature) :-(where a = initial concentration)(1) t × a = constant, for 2 order kinetics(2) t × a = constant, for I order kinetics(3) t × a = constant, for zero order kinetics(4) Unit of rate constant is M sec for I order

Question

Solution

Similar Questions

Upgrade your grade with Knowee