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For the gaseous reaction: N(2)O(4) rarr ...

For the gaseous reaction: `N_(2)O_(4) rarr 2NO_(2)`

A

`DeltaH gt DeltaU`

B

`DeltaH lt DeltaU`

C

`DeltaH = DeltaU`

D

`DeltaH = 0`

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To solve the problem regarding the gaseous reaction \( N_2O_4 \rightarrow 2NO_2 \) and the relationship between the changes in enthalpy (\( \Delta H \)) and internal energy (\( \Delta U \)), we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Reaction**: The reaction given is: \[ N_2O_4 \rightarrow 2NO_2 \] ...
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For the reaction : 2N_(2)O_(5) rarr 4NO_(2) +O_(2) , the rate of reaction in terms of O_(2) is d[O_(2)] /dt. In terms of N_(2)O_(5) , it will be :

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Following data are obtained for the reaction: N_(2)O_(5) rarr 2NO_(2) + .^(1//2) O_(2) |{:(t//s,0,300,600),([N_(2)O_(5)]//mol L^(-1),1.6 xx 10^(-2),0.8 xx 10^(-2),0.4 xx 10^(-2)):}| (a) Show that it follows first order reaction (b) Calculate the half-life (Given log 2 = 0.3010 log 4 = 0.6021]

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)rarr4NO2_(g)+O_(2)(g) if the concentration of NO_(2) increases by 5.2xx10^(-3)M in 100 sec, then the rate of reaction is :

For the reaction : 2N_(2)O_(5)rarr4NO_(g)+O_(2)(g) if the concentration of NO_(2) increases by 5.2xx10^(-3)M in 100 sec, then the rate of reaction is :

What is the activation energy for the reverse of this reaction? N_(2)O_(4)(g)rarr2NO_(2)(g) Data for the given reaction is : DeltaH=+54 kJ and E_(a)=+57.2kJ :

The rate constant for the reaction, 2N_(2)O_(5) rarr 4NO_(2) + O_(2) is 3.0 xx 10^(-5) s^(-1) . If the rate is 2.40 xx 10^(-5) mol L^(-1) s^(-1) , then the initial concentration of N_(2)O_(5) (in mol L^(-1) ) is

The decompoistion of N_(2)O_(5) in C CI_(4) solution at 318 K has been studied by monitoring the concentration of N_(2)O_(5) in the solution. Initially, the concentration of N_(2)O_(5) is 2.33 M and after 184 min , it is reduced to 2.08 M . The reaction takes place according to the equation: 2N_(2)O_(5) rarr 4NO_(2) + O_(2) Calculate the average rate of this reaction in terms of hours, minutes, and seconds. What is the rate of Production of NO_(2) during this period?

CENGAGE CHEMISTRY ENGLISH-THERMODYNAMICS-Exercises (Single Correct)
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