Assignment:
Question 1. Consider the following reaction: 2N2O(g) →2N2(g) + O2(g)
a. Express the rate of the reaction with respect to each of the reactants & products.
b. In the first 10s of the reaction, .018 mol of O2 is produced in a reaction vessel with a volume of .250L. what is the average rate of the reaction over this time interval?
c. Predict the rate of change in the concentration of N2O over this time interval. In other words, what is delta[N2O]/delta t ?
Question 2. Consider the following reaction: NO2 →NO(g) + 1/2O2(g) the following data were collected for the concentration of NO2 as a function of time:
time(s): 0, 10, 20, 30, 40, 50, 60, 70, 80, 90, 100
[NO2]: (M) 1.0, .951, .904, .860, .818, .778, .740, .704, .670, .637, .606
a. What is the average rate of the reaction between 10 and 20s? between 50 and 60s?
b. What is the rate of formation of O2 between 50 and 60s?
Question 3. A reaction in which A, B, and C react to form products is zero order in A, one half order in B, and second order in C.
a. Write a rate law for the reaction.
b. What is the overall order of the reaction?
c. By what factor does the reaction rate change if [A] is doubled? (and the others are constant)
d. By what factor does the reaction rate change if [B] is doubled? (and the others are constant)
e. By what factor does the reaction rate change if [C] is doubled? (others are constant)
f. By what factor does the reaction rate change if the concentration of all 3 reactants are doubled?
Provide complete and step by step solution for the question and show calculations and use formulas.