The rate of change of molar concentration  of N2O5 gas in the following reaction was reported as d[N2O5]/dt = -1.5 dm^-3 s^-1 under particular  conditions.  2N2O5 (g) = 4NO2 (g) + O2 (g)  Calculate   (a) the rate of reaction  (b) the rate of formation  of O2.

(a) Suppose the rate of formation of Br2 is 4.0 x 10° M/s in a reaction in water described by the following net ionic equation: 5Br +BrO3¯ + 6H* → 3B12 + 3H20. What are the rates of reaction of each of the reactants and the reaction velocity? 14. (b) List two possible scenarios that may lead to zero-order reactions.

The activation energy for the isomerization reaction CH3NC(g) → CH3CN(g) is 161 kJ mol−¹, and the reaction rate constant at 600 K is 0.41 s¯¹. (a) What is the value of the pre-exponential factor A for this reaction? (b) What is the value of the rate constant of the reaction at 1000 K?

Choose the correct molecularity and rate law for each of the elementary reactions shown below. (a) Cl(g) + CCl3(g) CCl4(9) Molecularity: ---Select--- V (b) SO3(9) SO₂(g) + 0(g) Molecularity: ---Select--- (c) NO₂(g) + SO₂(g) NO(g) + SO3(9) Molecularity: ---Select--- (d) 2 NO₂(g) N₂04(9) Molecularity: ---Select--- (e) CH₂OOCH3(g) 2 CH₂O(g) Molecularity: ---Select--- Rate Law: Rate = k [CC14]² Rate = k [CI] [CC13] Rate = k [CI]² [CC13]² Rate = k [CCl4] Rate Law: Rate = k [S0₂] [0] Rate = k [SO3] Rate = k [SO3]² O Rate = k [S0₂]² [0]² Rate Law: O Rate = k [NO₂] [SO₂] Rate = k [NO₂]² [S0₂]² O Rate = k [NO]² [S03]² O Rate = k [NO] [S03] Rate Law: O Rate = k [NO ₂] Rate = k [N₂04]² Rate = k [N₂04] O Rate = k [NO₂]² Rate Law: O Rate = k [CH30] Rate = k [CH300CH3]² Rate = k [CH30]² Rate = k [CH3OOCH3]

The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(g) +SİH4(g)–→HI(g) +SIH3I(g) The activation energy is Ea = 83.2 kJ mol-1. At 269°C, the reaction rate constant is 3.49 L mols. (a) Calculate the Arrhenius factor A for this reaction. L mols1 (b) Calculate the rate constant for this reaction at 235°C. L molls1

Writing the rate law implied by a simple mechanism Suppose the formation of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 2 NO(g) → N,O2(9) 2 N2O2(9) + O2(9) → 2 NO,(9) olo Suppose als0 k, «k,. That is, the first step is much slower than the second. Write the balanced O-0 chemical equation for the overall chemical reaction: 믐 Write the experimentally- observable rate law for the overall chemical reaction. rate = k || 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. ||

The differential rate laws for the balanced chemical reaction: aA(aq) + bB (aq) + CC (aq) → product is given by: raterxn = k [A]³[C]³ [B]³ What are the order in each chemical, as well as the overall order of the chemical kinetics? Place your answer in each box, respectively! Provide detailed solution (The order of kinetics in A) = (The order of kinetics in B) = (The order of kinetics in C) = (The overall order of kinetics) =

13.74 Methyl acetate, CH,COOCH3, reacts in basic solu- tion to give acetate ion, CH;COO , and methanol, CH,OH. CH,COOCH,(ag) + OH (ag) → CH;COO (ag) + CH;OH(aq) The overall order of the reaction was determined by start- ing with methyl acetate and hydroxide ion at the same con- centrations, so [CH,COOCH3] = [OH]= x. Then Rate = k[CH,COOCH;"[OH¯]" = kx"*n %3D %3D Determine the overall order and the value of the rate con- stant by plotting the following data assuming first- and then second-order kinetics. Time (min) [CH,COOCH;] (mollL) 0.00 0.01000 3.00 0.00740 4.00 0.00683 5.00 0.00634 10.00 0.00463 20.00 0.00304 30.00 0.00224

The rate of the reaction A + 3 B → C + 2 D was reported as 2.7 mol dm−3 s−1. State the rates of formation and consumption of the participants.

At 400 K, the rate of decomposition of a gaseous compound was 9.71 Pa s−1 when 10.0 per cent had reacted and 7.67 Pa s−1 when 20.0 per cent had reacted. Identify the order of the reaction.