The photochemical chlorination of chloroform, CHCI3 + Cl2 – CCI4 + HCI is believed to proceed by the following mechanism: Ch + hv 2CI Cl + CHC!3 ki CCI3 + HCI k2 CCI3 + C2 CCI4 + CI 2CCI3 + C2 k3 2CCI4 Derive the steady-state rate law for the production of carbon tetrachloride.

For a gaseous mixture of N2, H2 and NH3 with no catalyst present (so that the rate of reaction is zero), (i) identify and state the number of component(s), phase(s) and degree of freedom. (ii) Provide reasonable choice(s) for the independent intensive variable(s).

A reaction profile (not to scale!) for the reaction CH4 + HCIC,H;Cl is shown below: E (kJ) 205 C2H4 + HCI 70 C2HSCI Reaction Coordinate Which of the following are true? Choose ail that apply. O AE is positive. | The energy of the products is lower than the energy of the reactants. | The value of Ea in the presence of a catalyst would be larger than 205 kJ. | The magnitude of Ea for the reverse reaction is larger than 205 kJ. O The value of AE in the presence of a catalyst would be smaller than -70.0kJ

The reduction of nitric oxide with hydrogen 2 NO + 2 H2N2 + 2 H20 is second order in NO and first order in H2. Complete the rate law for this reaction in the box below. Use the form k[A]"B"... , where '1' is understood for m, n. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.58 M-?s1. Using this value for the rate constant, the rate of the reaction when [NO] = 0.328 M and [H2] = 0.363 M would be |Ms-!.

A mechanism that has been proposed for the conversion of 2-methylpropene to tert-butyl alcohol in acidic aqueous solution is: step 1 slow: (CH),С-СH,+ н* — (CH);с* step 2 fast: (CH;)3C* + H,O → (CH3);COH + H* (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]m[B]"... , where 'l' is understood (so don't write it) for m, n etc.) Rate =

The ozonization of pentene in carbon tetrachloride solution at 25 °C C3H10 + O3C3H10O3 is first order in C3H10 and first order in O3. Complete the rate law for this reaction in the box below. Use the form k[A]"B"... , where '1' is understood for m, n. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 250 Ms-1 when [C3H10] = 9.52×10-2 M and [O3] = 2.41×10-² M. From this experiment, the rate constant is

Please don't provide handwritten  solution...

For the gas phase decomposition of 2-bromopropane,CH3CHBrCH3CH3CH=CH2 + HBrthe rate constant in s-1 has been determined at several temperatures. When ln k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.55×104 K and a y-intercept of 29.9.The value of the rate constant for the gas phase decomposition of 2-bromopropane at 675 K is _____ s-1.

The oxidation of SO2 to SO3 is accelerated by NO2. The reactionproceeds according to:NO2(g) + SO2(g)---> NO(g) + SO3(g)2 NO(g) + O2(g)--->2 NO2(g)(a) Show that, with appropriate coefficients, the two reactionscan be summed to give the overall oxidation of SO2by O2 to give SO3. (b) Do we consider NO2 a catalyst or anintermediate in this reaction? (c) Would you classify NOas a catalyst or as an intermediate? (d) Is this an exampleof homogeneous catalysis or heterogeneous catalysis?

The reaction of tertiary butyl bromide with hydroxide ion at 55 °C (CH3)3 CBr + OH- = (CH3)3 COH + Br-  is first order in (CH3)3 CBr and first order overall. Complete the rate law for this reaction in the box below. Use the form , k ;[A]m [B]n where '1' is understood for  or  and concentrations taken to the zero power do not appear. Don't enter 1 for m  or .n Rate =