Answer Happy

1. [20 pts] The ammonium ion (NH4+)
reacts with nitrite ion (NO2-) to yield
nitrogen gas and liquid water. The following initial rates of
reaction have been measured for the given reactant
concentrations:
Write the balanced chemical equation [2 pts]
Deduce the empirical rate law from the data [10 pts]
What is the rate of the reaction of the concentrations of both
ammonium and nitrite ions are 0.010 M each [3 pts]
2. [15 pts] The rate constant for the first-order
reaction: SO2Cl2(g) = SO2(g) +
Cl2(g) is 2.2 x
10–5 s --1. Assume that the initial
concentration of SO2Cl2 is 2.00 M.
A. What is the half-life? [5 pts]
B. How long would it take for the concentration of
SO2Cl2 to decrease to 25% of its initial
value? [5 pts]
C. How long will it take for 12.5% of its initial value to
decompose? [5pts]
3. [10 pts] The decomposition of nitrogen dioxide:
2NO2(g) = 2NO(g) + O2(g) has a rate
constant of 0.498 M/s at 592 K and a rate constant of 1.81 M/s at
627 K.
A. [5 pts] Estimate the value of the activation energy for
this reaction.
B. [5 pts] What is the rate constant at 600 K?