Answer:-
This question is solved by using the simple concept of chemical kinetics which involves the rate of reaction determination.
The answer is given in the image,
. Determine the rate law, including the rate constant (with correct units) for the following reaction:...
A reaction between substances A and B has been found to give the following data:3A + 2B --> 2C + D[A] (mol/L)[B] (mol/L)Rate of appearance of C (mol/L-hr)1.0 x 10^-21.00.3 x 10^-61.0 x 10^-23.08.1 x 10^-62.0 x 10^-23.03.24 x 10^-52.0 x 10^-21.01.20 x 10^-63.0 x 10^-23.07.30 x 10^-5
3. For the reaction C3H3(g) + 5 O2(g) ----> 3 CO2(g) + 4H20(1) the following rate data were determined at 30°C. Experiment Initial C3H8 Initial O2 id. Rate 0.200M 0.200 M 3.00 x 101 0.400 M 0.200 M 6.00 x 101 0.200 MO 0.400 M 1 .20 x 102 a) Determine the reaction order with respect to C3H8. b) Determine the reaction order with respect to 02. c) Calculate the rate constant at this temperature. d) Write the rate law...
7. What is the reaction order for each reactant and the rate coefficient for the following reaction? A+B+C ->Z [A] (mol L B (mol L[C] (mol L ](mol L sec1) 0.010 0.020 0.010 0.020 0.0100 0.0100 0.0200 0.0100 0.10 0.10 0.10 0.20 3.0 x 10-2 3.0 x 102 1.2 x 10-1 1.5 x 10-2
5. (15 pts) Determine the rate law and rate constant for the following reaction 2A + B + 2CD + 2E Given Experiment [A], mol/L [B], mol/L [C), mol/L 1 2 1.5 3.0 3.0 1.5 1.5 1.5 3.0 1.5 الم Rate, mol/L) 0.255 1.10 2.30 0.240 1.5 1.5 1.5 3.0 4
1)The rate law of a reaction is rate =k[X]³. The units of the rate constant areL mol-1 s-1mol² L-2 s-1mol L-1S-2L² mol-2 s-1mol L-1S-12)Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate =k[X]³[Y]²[Z]⁰The rate of reaction will increase by a factor of136803)What data should be plotted to show that experimental concentration data fits a first-order reaction?1 / [reactant] vs. time[reactant] vs. timeln (k) vs. Ealn (k) vs. 1 / Tln [...
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02 DU 3. The reaction below gave the following data in an experiment that was NOT well-designed. OH- ClO-(aq) + (aq) ---> Cl(aq) +10-(aq) Initial concentrations Trial (CIO), M [1],M [OH-], M Initial Rate, M/s 2.0 x 10-3 2.0 x 10-3 1.00 2.42 x 10-4 3.0 x 10-3 2.0 x 10-3 1.00 3.60 x 10-4 4.0 x 10-3 4.0 x 10-3 1.00 9.40 x 10-4 2.0 x 10-3 2.0 x 10-3 0.50 4.75 x 10-4...
9. Given the initial rate data below, what is the rate law for the following reaction? 2CIO2(aq)2OH (aq) > CIO3 (aq) CIO2 (aq) H20 [ОН 1о (mol L) Initial rate [CIO2lo (mol L) (mol L s 0.100 0.100 0.23 0.200 0.050 0.46 0.200 0.100 0.92 b) rate k[CIO2][OH] e) rate k[CIO2]3 c) rate [CIO2]OH 12 a) rate k[CIO2][OH ] k[CIO2] [OH] = d) rate = 13I to drop to 95% of its initial value? The 10. How long does it...
2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the data provided: 2 NO (g) + 02 (g) > 2 NO2 (g) Rate (M/s 0.028 0.057 0.114 0.227 Experiment NO 0.020 0.020 0.020 0.040 0.010 0.010 0.020 0.040 0.020 0.020 3 4 a.) For the rate law, determine all reaction orders Rate -k [NO]m[O2]' Reaction order m (CIRCLE ONE) 1½ Reaction order n (CIRCLE ONE) 1½
Given the reaction and following data: 2NO + O2 → 2NO2 Calculate the rate law constant and write the rate law. Trial [NO] (mol/L) [O2] (mol/L) Rate (mol/L/hr) 1 0.125 0.125 2.57 x 10-2 2 0.250 0.125 5.20 x 10-2 3 0.250 0.250 4.16 x 10-1
The rate law for the reaction 2NO28) 2NO(8) +02(3) is IS rate k [NO212. Initially, only NO2 was present in the reaction vessel and its concentration was 7.48 x 10-4 mol/L 312 minutes after the reaction started the concentration of 02 was determined to be 2.92 x 104 mol/L. Determine the time required for the concentration of NO2 to drop to 5.28 x 10-4 mol/L O 83.2 min 203 min 536 min O616 min 754 min