The below reaction follows second order rate kinetics and proceeds via a bimolecular mechanism. KCNCH3B1 -» KBr + CH3CN If the concentration of potassium bromide were doubled, how many times faster would the reaction go? If the concentration of CH3Br were doubled. How much faster would the reaction go? Write the rate law for the above reaction. If [KCN] 0.5 M, [CH3Br] 0.5 M, and the relative reaction rate is 0.25 M/s, what is the rate constant? Also, what are the units of the rate constant?

Write a balanced reaction for which the following rate relationships are true.Rate = -1/2Δ[N2O5]/Δt=1/4Δ[NO2]/Δt=Δ[O2]/Δt

Which of the following is an (are) intermediate(s) in the mechanism of the reaction shown below.

rate expression: rate = k[H2O2]m[I-]n 1. Would your specific rate constant, k, be larger than, smaller than, or unchanged from the correct value as a result of each of the following mistakes? Justify your answers. a) You accidentally substituted a value for n twice as great as it should have been when calculating k. b) Your water bath in the 600-mL beaker was about 5ºC warmer than room temperature for all three of your experiments.

For the reaction   2NO + Cl2  ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above            NO + Cl2  NOCl2     fast equilibriumNOCl2 + NO  2NOCl     slow            2NO  N2O2     fast equilibriumN2O2 + Cl2  2NOCl     slow            Cl2  2Cl     slowCl + NO  NOCl     fast            NO + Cl2  NOCl + Cl     slowCl + NO  NOCl     fast

Please describe what would happen to the rate if given changes were applied to following reactions: Ex.: Doubling the concentration of both KOH and starting material in the reaction below Br OH KOH It is a 2nd order reaction. Doubling the concentration of both will result in 4x the speed of the reaction. DMF 1. Doubling the concentration of starting material and alcohol in the reaction below Br Br CH3OH 2. Using half of the alcohol in the reaction shown below CH3OK CH3OH

Which of the following rate laws has an overall reaction order of 1? rate= k[CO]° rate= k[H2O2] rate= k[H*][OH"] O rate= k[H2O2]²

The activation energy for the gas phase decomposition of cyclobutane is 262 kJ. (CH₂) 4- →2 C₂H4 The rate constant at 721 K is 0.000401 /s. The rate constant will be 0.00338/s at K.