2NO+2H2=2H2O+N2 If Δ[NO]/ Δt = –22.0 M/s under a given set of conditions, what are the rates of change of [N2] and [H2O]?

2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all  the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for  the reaction at 625 K.

Chlorine monoxide (ClO) accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, ClO decomposes according to the equation: 2C1O (g) → Cl2 (g) + O2 (g) The kinetics of this reaction were studied in a laboratory experiment at 298K, and the data are shown in the table below. (a) Determine the order of the reaction (b) Determine the rate law expression (c) Determine the value of the rate constant, k, at 298K. Time (ms) [CiO] (M) In [ClO] cioj (M-1) [CiO] 6.67 × 107 1.39 x 108 -8- 1.50 x 10 7.19 x 10 4.74 × 10 -18.0 6- 10 -18.8 6- 20 -19.2 2.11 x 108 6- 30 3.52 х 10° -19.5 2.84 x 108 6- 40 2.81 x 10 -19.7 3.56 x 108 6- 100 1.27 x 10 -20.5 7.87 x 108 10 200 6.60 x 10- -21.1 1.52 x 10°

Consider the mechanism: NO2(8) + SO2(g) → NO(g) + SO3(g) NO(g) + ½ O2(g) –→ NO2(g)

Reaction of nitric oxide gas (NO) and chlorine gas (Cl2) produces a very poisonous gas called nitrosyl chloride (NOCl). The experimental data of the reaction is given below. Use the data to calculate the specific rate constant K and overall order of the reaction. Please show full work!

The rate constant of a chemical reaction increased from 0.100 s−1 to 3.20 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C . Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.