The following mechanism for the gas phase reaction of nitrogen dioxide with carbon monoxide at temperatures above 225 °C is consistent with the observed rate law. step 1: NO₂ + CO→→→→→→→ ONOCO step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 ONOCO NO + CO2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (c) Identify any intemediates in this mechanism. Intermediate: Enter formula. If none, leave box blank:

(4) Use the following experimental data to write the rate law and the rate constant for the reaction 2 NO (g) + O2 (g) = 2 NO2 (g) Experiment [NO] (M) [O2] (M) Initial rate (M/s) 1 0.0100 0.0100 0.711 x 10-2 2 0.0100 0.0400 2.84 x 10-2 3 0.0200 0.0100 2.84 x 10-2

The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?

Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first-order process to methane and ketene (CH2═C═O). At 600°C, the rate constant is 8.7 × 10−3 s−1. (a) What is the half-life of the reaction? Give your answer in scientific notation. (b) How long does it take for 38% of a sample of acetone to decompose?  (c) How long does it take for 81% of a sample of acetone to decompose? Give your answer in scientific notation.