Question

1. Calculate the activation energy, Ea, in kilojoules per mole for a reaction at 73.0 ∘C that has a rate constant of 0.278 s−1 and a frequency factor of 9.74×1011 s−1.

Ea= kJ/mol

2.

Nitogen dioxide, NO2, is a red-brown gas that is considered an air pollutant. When heated, nitogen dioxide gas decomposes into nitrogen monoxide and oxygen gas, according to the following reaction.

2NO2(g)−⇀↽−2NO(g)+O2(g)

A sample of nitrogen dioxide in a sealed vessel was heated to 575 K, and the total pressure in the vessel was measured to be 0.0980 atm before any reaction had occured. The total pressure in the vessel was monitored over time during the reaction, giving the following data.

Time (s)	Total pressure (atm)
0	0.0980
23	0.1249
57	0.1348
95	0.1389

What is the rate law for the decomposition reaction?

a. rate=kPNO2

b. rate=kPNOPO2

c. rate=k

d. rate=kP2NO2

Calculate the rate constant for the reaction. Determine the units on the rate constant based on the order of the reaction.

k=

units:

Determine the total pressure in the reaction vessel after 386 s.

Ptotal= atm

Answer 1

STRANI According to Arrhenius of equation, K . A. karate constant = 0.27851 Az Frequerey factor = 9.74x10''sec! Ra Gas constant = 8.314 3/molk T2 Temperature = (273+73) K = 346k Ea= Activation energy. so 0.278 = 9.74x10". é 80/8.3148346 » è to/2876.64 = 2.85 x 10-13 - aby = lon (2-85x1013) = -28.88 - s Ea=83091.20 J 283.0912 kJ So the activation energy is 83.0912 kJ/mol WALI S 1.