Consider this initial rate data at a certain temperature in the table for the reaction [OCI-], [OH-]o Initial rates OH (aq) OCI (aq) +I (aq) OI (aq) + Cl (aq) Trial (М) (М) (M/s) (М) 1 0.00185 0.00185 0.450 0.000494 0.00185 0.00324 0.450 0.000864 3 0.00350 0.00185 0.621 0.000676 4 0.00185 0.00324 0.653 0.000596
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- Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.360 0.290 0.0144 2 0.360 0.580 0.0144 3 0.720 0.290 0.0576 k=Part B: Integrated rate law expressions for zero- and half-order reactionsDerive integrated rate law expressions for half-, one and a half-, and third-order reactions of the form A products where k is the rate constant. Also, deduce the graphical linear relations, units of rate constant k, and expression for half-life, t1/2 , for all cases. Assume that at t = 0 only A is present with an initial concentration of [A]0. Fill in the table below by following the example given for first-order reaction1.
- Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=Given the following data, determine the rate law and calculate K Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4 the units on K are M-2s-1. You should enter the answer without units to 2 sig figs.Consider the base hydrolysis of an ester.RCOOR' + OH− → RCOO− + R'OH (where R and R' represent organic groups).The kinetics of this reaction, for a particular ester, were studied using the isolation method. When [OH−] << [RCOOR'] a pseudo-rate law can be posed:-d[OH-] / dt = k'' [OH-]mWith initial concentrations: [OH−]0 = 0.0015 M [RCOOR']0 = 0.700 M a plot of ln[OH-] versus t gave a straight line with slope = -0.0176 s-1 and y-intercept = -6.50.What is the order "m"?m = ? What is the corresponding pseudo rate constant k''? (include appropriate units)k'' = ?
- For the gas phase decomposition of cyclobutane,(CH2)4----->2 C2H4the 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 -3.15×104 K and a y-intercept of 35.9.The value of the rate constant for the gas phase decomposition of cyclobutane at 711 K is _____ s-1.(Enter your answer to one significant figure.)The following results were found after completion of Part C in the Experimental procedure: 0.057 M I- and 0.065 M H2O2 were used Run Catalyst Calculated Rate of Reaction (M/s) 1 none 0.053 2 10.00mL of 0.54 M FeCl2 0.446 Assuming the Rate Law = k[I-][H2O2] 2 Calculate the value of k for run 2. Give your answer to the nearest whole number.Fill in the table with the correct responses. Reaction Order Integrated Rate Law Linear Plot Rate constant (k) from the linear plot Half life (t1/2) zero [a] [b] [c] [d] first [e] [f] [g] [h] second [i] [j] [k] [l] Answer bank: 1/At = kt + 1/Ao ln A vs time negative of the slope (-m) log A vs time At = -kt + Ao At/k Ao/2k y-intercept A vs time slope (m) At = kt + Ao 1/A vs t lnAt = -kt + lnAo ln2/k 1/kAo
- Given the following data, determine the rate law and calculate K Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4 the units on K are M-2s-1. You should enter the answer without units to 2 sig figs. Enter only the numerical value of KUsing the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?)[) Rate (M/s) 1 0.370 0.390 0.0234 2 0.370 0.936 0.135 3 0.592 0.390 0.0374 ?= ? units= ?In Experiment 4- Chemical Kinetics “The Rate of Chemical Reaction”, the following data were obtained: Rxn Mixture time(s) temperature (˚C) 1 190 23.0 2 378 23.0 3 97 23.0 4 205 23.0 5 44 23.0 6 90 35.0 Concentrations and portions for reaction mixture number one: H2O 0.050 M Buffer 0.050 M KI (mL) 0.1% Starch (mL) 0.0450 MNa2S2O3(mL) 0.8525 M H202 (mL) 75.0mL 30.0mL 25.0 5.00 5.00 10.00 Use the data above to answer the following questions where applicable. (a) Write the formulas of the reactants, there are three, in the reaction being studied.Signs + or - or subscripts may be entered all on the same line; S2O32- can be entered as S2O3^2-, the symbol, ^, is not required if the…