Question

The following data were obtained for the decomposition of N2O5 in CCl4 at 45 °C:

a. What is the order of the reaction with respect to (WRT) dinitrogen pentoxide?
b. What is the value of k?
c. What is the value of the half-life for the reaction in minutes?

Answer 1

a)
`k = (ln(C_0)/(C_t) )/(t) \\k = (2.3)/(t) log (C_0)/(C_t)`

b)
`6.31 * 10^(-4)`

c)
`1.094 * 10^(-3)`

Step-by-step explanation:

Complete question

(min) 0 135 342 683 1693

c {M} 2.08 1.91 1.67 1.35 0.57

Solution -

a) One this clear from the data provided and it is that rate of the reaction does not remain constant with time and hence it is not a zero order reaction. Thus, the equation for first order reaction is

`k = (ln(C_0)/(C_t) )/(t) \\k = (2.3)/(t) log (C_0)/(C_t)`

b) Rate of reaction

Substituting the given values in above equation, we get -

`k = (2.3)/(135) log (2.08)/(1.91) \\= 6.31 * 10^(-4)`

c) Value of the half-life for the reaction in minutes

`t_{(1)/(2)} = (0.69)/(k)`

Substituting the given values in above equation, we get -

`t_{(1)/(2)} = (0.69)/(6.31 * 10^(-31)) \\t_{(1)/(2)} = 1.094 * 10^(-3)`

per minute