Consider the bimolecular reaction of nitrogen dioxide at 750 K in the gas phase, producing NO and O2 as follows: 2NO22NO + O2. Suppose that the Arrhenius parameter (frequency factor A) is given as 1.79 x 106 m³ mol¹ s¹ and the actual cross-section for a reactive collision is σ = 0.60 nm². Calculate the reactive cross section (σ*) and the steric factor, P. HINT: take μ = 1/2m(NO2) And MNO2 = 46.0mu, where mu is the atomic mass constant.

Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.

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.

The specific rate constant for the first-order decomposition of -1 N₂O5 (9) to NO2 (g) and O₂ (g) is 7.48 × 10-³ s¯ at a given temperature. Find the length of time required for the total pressure in a system containing N₂O5 at an initial pressure of 0.110 atm to rise to 0.150 atm . Express your answer using two significant figures. VE ΑΣΦ t = Submit Part B t = Submit Request Answer Find the length of time required for the total pressure in a system containing N₂O5 at an initial pressure of 0.110 atm to rise to 0.220 atm . Express your answer using two significant figures. ΨΕ ΑΣΦ Part C Request Answer ? Find the total pressure after 120 s of reaction. S S

In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)2 NO,(g) + ½ O2(g) the concentration of N2O5 was followed as a function of time. It was found that a graph of In[N,O3] versus time in seconds gave a straight line with a slope of -7.38×10-3 s and a y-intercept of -3.13. Based on this plot, the reaction is | order in N2O5 and the half life for the reaction i | seconds.

It has been proposed that the gas NO2C1 decomposes by the mechanism: NO2CI(g) kı NO2(g) + Cl(g) NO2CI(g) + Cl(g) k2 NO2(g) + Cl2(g) Apply the Steady State Approximation to derive an expression for the concentration of the intermediate, Cl(g). Show your working out. States not required.

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.