The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y. (b) the rate constant? For the experiments (a) [Y] = 2. 7 mmol dm-3 and for experiments (b) ]Y] = 6.1 mmol dm-3[complex]/(mmol dm-3)            8.01    9.22    12.11v/(mol dm-3 s-1) (a)                   125     144     190                           (b)                   640     730     960

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]

[4] The reaction: 21 (aq) + S2O;²-(aq) → I½(aq) + 2SO,²-(aq) is first order with respect to I and first order with respect to S20g. The rate constant k was determined at different temperatures and a plot of In(k) versus 1/T was constructed resulting in the straight line: y = -5781.8x + 14.1. Assume k has units of M's. (a) Determine the activation energy for this reaction. (b) Calculate the value of k at 20 °C.