Starting with [CV] = 1.0x105 M and [NaOH]; = 0.050 M, a set of their reaction kinetics data was collected over 3 minutes and plotted as shown below, In[CV+] -11.4 -11.6 -11.8 -12 -12.2 -12.4 -12.6 -12.8 0 20 40 Crystal Violet Kinetics First Order Rateo k[CV]o = 60 80 100 time (sec) k = 120 140 160 y = -0.0059x11.587 R20.9987 The line fit data are represented by the first-order integrated rate law: [CV] = [CV]oekt Use the values obtained by the line fit of [CV*]o and k from for all the following calculations. Write these parameters below, rounded to 2 significant figures with units! [CV] = 180 200 Is the concentration of crystal violet at the time of mixing identical to the initial concentration calculated from the graph (at the beginning of data collection)? Why? Calculate the instantaneous rate of crystal violet consumption at the beginning of the data collection, t = 0 seconds.

[Review Topics] [References] Use the References to access important values if needed for this question, A reaction profile (not to scale!) for the reaction H, + I,2 HI is shown below: E (kJ) 171 H2 + 12 13 HI + HI Reaction Coordinate This reaction is (exothermic,endothermic) The value of the activation energy for this reaction is kJ and the value of AE is kJ. Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning | Cengage Technical Support 98°F Rain comi

The rate expression for the reaction between H2O2 and KI is:rate = k[H2O2]m [KI]nwhere: k = rate constantm = order of reaction with respect to H2O2n = order of reaction with respect to KI   Table 2:  Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Order with respect to H2O2: -0.138 Order with respect to KI: -0.828   Rate constant value                         Trial 1: 5.84                         Trial 2: 5.55                         Trial 3: 5.56                         Average: 5.6 -Please help me with this part, please 1.Write the complete rate law for this reaction. 2.List two sources of error for this experiment.

The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: OCr +I- OI + CI Experiment [OCI"]o, M , M Initial Rate, Ms™ -1 1.70×10-3 1.70×10-3 3.40x10-3 3.40x10-3 4.57×10-3 9.15×10-3 4.57x10-3 9.15×103 1 5.41x10-4 1.08×10-3 1.08×10-3 2.17x10-3 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M's.

For a first-order reaction k A + B time t = 0 s 4.878 1.004 M time t = 19.84 s ? M when k = 0.030329 s-1 what is the concentration of B above in the question mark= _M? 3 sig. fig. normal format. Try to plot concentrations of A, B and rate over time in Excel.

Use the attached data to plot a graph "ln a as a function of time" for both 20ºC and 30ºC. Use the equation: y=-mx +b where y is ln a, m is k, x is time. Does this poor confirm a first order reaction? If so, how do you know?

The rate expression for the reaction between H2O2 and KI is:rate = k[H2O2]m [KI]nwhere: k = rate constantm = order of reaction with respect to H2O2n = order of reaction with respect to KI   Table 2:  Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20     please help me with this part and please show me all steps    Rate constant value                         Trial 1 ______________                         Trial 2 ______________                         Trial 3 ______________                         Average _____________

it is not graded!!!!

Please help, thanks.

Use the References to access important values if needed for this question. The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g)NO(g) + % Ch(g) is second order in NOCI with a rate constant of 5.90x10-4 M's!. If the initial concentration of NOCI is 0.116 M, the concentration of NOCI will be 1.43x102 M after seconds have passed.