Decomposition of N2O5 follows first order kinetics and its instantaneous rate is 1.6 x 10^-6 mol/L/s. Calculate the rate constant of the reaction of 0.02M solution.

8×10^-5 s^-1

Explanation:

The decomposition of N2O5 is shown by the reaction equation;

N2O5(aq)⇄NO2(g) + NO3(g)

We have the following information;

Instantaneous rate of reaction = 1.6 x 10^-6 mol/L/s.

Concentration of the N2O5 = 0.02M

Now the rate of decomposition of N2O5 is given by;

R= k[N2O5] (first order reaction)

Hence;

1.6 x 10^-6 mol/L/s = k[0.02M]

k= 1.6 x 10^-6 mol/L/s / 0.02M

k= 8×10^-5 s^-1

Hence the rate of decomposition of N2O5 is 8×10^-5 s^-1

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

14 days is the half-life of phosphorus-32