Peroxyacetyl nitrate (PAN) has the chemical formula C2H3NO5 and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN.(base the table below):

The decomposition of hydrogen 2 peroxide is catalyzed by iodide ion. The reaction mechanism is thought to be H,O2(aq) + I(aq) → H,0(I) + 10(aq) 10(aq) + H,O2(aq) → H,O(I) + O2(g) + I(aq) At 25°C, the first step is slow relative to the second step. What is the rate law predicted by the reaction mechanism? Is there a reaction intermediate? 13 | 106

Consider the following reaction:2 SO2(g) + O2(g) → 2 SO3 (g)Write the relative rate expressions for all products and reactants in the order they appear in the written reaction.  If the rate of consumption of O2 is 0.90 mM/sec at some time in the reaction, what is the rate of formation of the SO3 at the same time in the reaction?

22.6a At 518°C, the half-life for the decomposition of a sample of gaseous acetaldehyde (ethanal) initially at 363 Torr was 410 s. When the pressure was 169 Torr, the half-life was 880 s. Determine the order of the reaction

Suppose the formation of nitrosyl chloride proceeds by the following mechanism: elementary reaction NO (g) + Cl₂(g) → NOC1₂ (g) k₁ k₂ 2 NOCI₂(g) + NO (g) 2NOCI (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. step 1 Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant ロ→ロ 00 × S

Consider the reaction : 3A + 2B →  4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 d. What is the order of the reaction. e. Express the rate law and the integrated form equation. Is the reaction elementary? f. If the rate constant k = 1.61x10-5s-1 and [A0] = 4M, find the period of time between the 12th and 13th half-life.   *g. If, for the same reaction, at the same temperature, we were to add a catalyst, would Ea, A, k and v be larger, smaller or equal? Explain.

The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first-order reaction: 4PH3(g) - P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. The first-order rate constant for the reaction is 0.0198/s. Calculate the time (in seconds) required for 95 percent of the phosphine to decompose.

The reaction between nitric oxide and bromine is described by the following chemical equation: 2NO (g) + Br, (g) – 2NOB (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) + Br, (g) NOB12 (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.

In a study of the decomposition of nitrous oxide at 565 °CN2O(g)N2(g) + ½ O2(g)the following data were obtained: [N2O], M 2.10 1.05 0.525 0.263 seconds 0 602 1.81×103 4.21×103 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 2.10 M is s and when the starting concentration is 1.05 M is s.(2)The average (1/[N2O]) / t from t = 0 s to t = 602 s is M-1 s-1.The average (1/[N2O]) / t from t = 602 s to t = 1.81×103 s is M-1 s-1.(3)Based on these data, the rate constant for this  order reaction is M-1 s-1.

The formation of nitrosyl chloride is described by the following chemical equation: 2NO (g) + Cl₂ (g) → 2NOCI (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) +Cl₂ (g) NOCI₂ (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 11 × Ś