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For the first order reaction 2N(2)O(5)...

For the first order reaction
`2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g)`

A

the concentration of the reactant decrease exponentially with time

B

the half-life of the reaction decreases with increasing temperature

C

the half-life of the reaction depends on the initial concentration of the reactant

D

the reaction proceeds to 99.6 % completion in eight half-life duration

Text Solution

Verified by Experts

The correct Answer is:
A, B, D
In first order reaction the half life do not depend upon initial concentration of the reactant.
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For the first order reaction. N_2O_5(g) rightarrow N_2O_4(g) + 1/2 O_2 (g), the volume of O_2 produced is 15 mL and 40 mL after 8 minutes and at the end of the reaction respectively. The rate constant is equal to

The initial concentration of N_(2)O_(5) in the following first order reaction: N_(2)O_(5)(g) rarr 2NO_(2)(g)+(1)/(2)O_(2)(g) was 1.24 xx 10^(-2) mol L^(-1) at 318 K . The concentration of N_(2)O_(5) after 60 min was 0.20 xx 10^(-2) mol L^(-1) . Calculate the rate constant of the reaction at 318 K .

For the reaction, 2N_(2)O_(5) (g) rarr 4NO_(2)(g) + O_(2)(g) , the rate of formation of O_(2) is 0.032 g h^(-1) . (a) Calculate the rate of converison of N_(2)O_(5) in g h^(-1) . (b) Calculate the rate of formation of NO_(2) in g h^(-1) .

The rate constant k , for the reaction N_(2)O_(5)(g) rarr 2NO_(2) (g) + (1)/(2) O_(2)(g) is 2.3 xx 10^(-2) s^(-1) . Which equation given below describes the change of [N_(2)O_(5)] with time ? [N_(2)O_(5)]_(0) and [N_(2)O_(5)]_(t) correspond to concentration of N_(2)O_(5) initially and at time, t ?

The rate constant k , for the reaction N_(2)O_(5)(g) rarr 2NO_(2) (g) + (1)/(2) O_(2)(g) is 2.3 xx 10^(-2) s^(-1) . Which equation given below describes the change of [N_(2)O_(5)] with time ? [N_(2)O_(5)]_(0) and [N_(2)O_(5)]_(t) correspond to concentration of N_(2)O_(5) initially and at time, t ?

For the reaction 2N_(2)O_(5)(g) to 4NO_(2) (g) + O_(2)(g) , the rate of formation of NO_(2)(g) is 2.8 xx 10^(-3) Ms^(-1) . Calculate the rate of disapperance of N_(2)O_(5)(g) .

For the first order reaction given below select the set having correct statements 2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g) (1) The concentration of the reactant decreases exponentially with time (2) the reaction proceeds to 99.6 % completion in eight half life duration (3) the half life of the reaction depends on the intial concentration of the reactant (4) the half life of the reaction decrease with increasing temperature

For the reaction 2NO_(2)(g)+(1)/(2)O_(2)(g)hArrN_(2)O_(5)(g) if the equilibrium constant is K_(p) , then the equilibrium constant for the reaction 2N_(2)O_(5)(g)hArr4NO_(2)(g)+O_(2)(g) would be :

The decomposition of N_(2)O_(5) according to the equation: 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) is a first order reaction. After 30 min. from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm of Hg and on complete decomposition, the total pressure is 584.5 mm of Hg. Calculate the rate constant for the reaction.

For a reaction, 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) rate of reaction is:

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