Consider the unimolecular reaction, CH3NC(g) = CH3NC(g), carried out in the presence of a helium buffer gas. The collision of a CH3NC molecule with either another CH3NC molecule or a helium atom can energize the molecule thereby leading to reaction. If the energizing reactions involving a CH3NC molecule and a He atom occur with different rates, the reaction mechanism would be given by CH3NC(g) + CH3NC(g) CH3NC*(g) + CH3NC(g) CH³NC(g) + He(g) — * — CH³NC*(g) + He(g) k3 CH3NC* (g) CH3CN(g) Apply the steady-state approximation to the intermediate species, CH3NC*, to show that k3(k₁[CH3NC]²+ k₂ [CH3NC] [He]) k₁[CH3NC] + k½ [He] + k3 rate = k₂ d[CH3CN] dt

(a) In the reaction mechanisms given, there are some chemical species which will get produced in one step and get consumed in the other step and that are not in reactants nor in products of the total reaction. Such species are known as intermediates of a reaction as the name suggests. Therefore, in mechanism 1, the intermediates are (CH3)2CHOH2+, Cl-, (CH3)2CH+. and in mechanism 2: (CH3)2CHOH2+, Cl-. These ions are neither reactants nor products of the given total equation.

Use the Referénces to access important values if needed for this question. The conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C CH3NC(g)→CH3CN(g) is first order in CH;NC. During one experiment it was found that when the initial concentration of CH;NC was 9.65×102 M, the concentration of CHąNC dropped to 1.43×10-² M after 436 s had passed. Based on this experiment, the rate constant for the reaction is Submit Answer Try Another Version 2 item attempts remaining Previous Nex

Consider the following proposed mechanismHBr + HBr ⇄ H2Br2(fast, equilibrium)HBr + R ⇄ ES(fast, equilibrium)H2Br2 +ES→P+2HBr(slow) (1a) What is the overall reaction? (1b) Identify all catalysts and intermediates in this reaction mechanism. (1c) What is the rate law derived from this mechanism? (1d) If the experimentally determined rate law is rate = k [HBr]3[R]1 what conclusion can be drawn? (1e) If the experimentally determined rate law is rate = k [HBr]2 what conclusion can be drawn? The equilibrium constant (KC) is 10.0 x 10-10 at

Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) Suppose also ≫. That is, the first step is much faster than the second. 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. 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 the reverse of the two elementary reactions in the mechanism.

At a certain temperature the rate of this reaction is second order in ClCH2CH2Cl with a rate constant of ·0.0543M−1s−1: →ClCH2CH2Clg+CH2CHClgHClg Suppose a vessel contains ClCH2CH2Cl at a concentration of 0.710M. Calculate the concentration of ClCH2CH2Cl in the vessel 210. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M

16.96 Experiment shows that the rate of formation of carbon tetrachloride from chloroform, CHCl3 (g) + Cl2 (g) → CCl4 (g) + HCl (g) 1 3 is first order in CHCl3, order in Cl₂, and order overall. Show that the following mechanism is consistent with the rate law: (1) Cl₂ (g)=2C1 (g) [fast] (2) C1 (g) + CHCl3 (g) → HCl (g) + CC13 (g) [slow] (3) CC13 (g) +Cl (g) → CC14 (g) [fast]

17) For the following reaction give the expression for the average rate for each species in the equation. 3 Ag₂S(s) + Al(s) + 3 H₂O(1)→6 Ag(s) + Al₂O3(s) + 3 H₂S(aq)

For the overall gas-phase reaction of the formation of phosgene (Cl₂CO) from carbon monoxide and chlorine, the following mechanism has been proposed: Cl₂ + M2CI+M k_1 CI+CO+MCICO + M k_2 k3 CICO + Cl₂C₁₂CO+CI Derive the expected rate law assuming [M] is large and constant, and using: (a) The equilibrium assumption for the first two steps. (b) Instead using the steady state assumption for any intermediates. (c) Why does the reaction become zeroth order in [CO] in the steady state case? (d) The actual rate law is 3/2 order in [Cl₂] and first order in [CO]. Which mechanism is likely correct? (e) Is the other mechanism possible, based on the observed orders?

Examine the curved arrow mechanism below, and answer the question in the box. If the mechanism is reasonable, draw all products. If the mechanism is not reasonable leave the drawing space blank. Is the curved arrow mechanism reasonable? O yes O no Click and drag to start drawing a structure. ?圖 图 ola Ar