Question

. At 25cC, gaseous dinitrogen pentoxide decomposes into the gaseous products nitrogen dioxide and oxygen. The product nitrogen dioxide has a reddish-brown color while both dinitrogen pentoxide and oxygen gases are colorless. The progress of the reaction can be followed by measuring the absorbance as the reddish-brown product accumulates. (a) Write a balanced net ionic equation with lowest whole number coefficients to describe the decomposition. (b) The reaction is found to be first-order. Which function of [N2O5] would give a straight line if plotted against time t

Answer 1

Answer:

2N2O5 (g) → 4NO2 (g) + O 2 (g)

Explanation:

2N2O5 (g) → 4NO2 (g) + O 2 (g)

The rate of reaction of N2O5 is first order with respect to dinitrogen pentaoxide. Hence the rate of reaction depends on change in the concentration of dinitogen pentaoxide.

This implies that for 2 N2O5(g) --------> 4 NO2(g) + O2(g), the rate of reaction is given by Rate = k[N2O5]

This implies that the rate of reaction plotted against time will give a straight line graph whose slope is the rate constant.