Homework Answers
Rate law
Rate = K[ClO2]^m[OH^-]^n
0.0575 = K(0.05)^m(0.1)^n -------------------------> 1
0.230 = K(0.1)^m(0.1)^n --------------------------> 2
0.115 = K(0.1)^m(0.05)^n ----------------------> 3
equation 1 divide by equation 2
0.0575/0.23 = K(0.05)^m(0.1)^n/ K(0.1)^m(0.1)^n
0.25 = (0.05/0.1)^m
(0.5)^2 = (0.5)^m
m = 2
equation 2 divide by equation 3
0.230/0.115 = K(0.1)^m(0.1)^n/ K(0.1)^m(0.05)^n
2 = (0.1/0.05)^n
(2)^1 = (2)^n
n = 1
Rate law
Rate = K[ClO2]^2[OH^-]^1
0.0575 = K(0.05)^2(0.1)^1
K = 0.0575/(0.05)^2(0.1)^1 = 230M^-2 sec^-1
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00 16t3 6. Consider the reachon Following rate nfo obtaincdl... m/S О. Ơ575 O.230 o. เ15...
Question 6 of 15 Submit A reaction has a rate law of Rate = (1.25 M-?s=')[A]...
Question 6 of 15 Submit A reaction has a rate law of Rate = (1.25 M-?s=')[A] [B]? What concentration of [B] would give the reaction a rate of 0.0891 if the concentration of [A] is 0.250 M?
thanks in advance ☺ (A). For the hypothetical reaction A+B → C the following rate data...
thanks in advance ☺
(A). For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s (A), M [B, M (uncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 4 7.14 x 10-2 0.100 0.100 1.75 x 104 7.14 x 10-2 0.0500 0.200 1.76 x 104 3.57 x 10-2 0.0500 0.100 8.80 x 10-5 3.57 x 10-2 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction,...
7. Consider the following reaction A+B - products. The rate law was found to be Rate...
7. Consider the following reaction A+B - products. The rate law was found to be Rate = k [A] [B]. Calculate k if [A] = 0.0500 M [B] = 0.125 M and the reaction took 405 seconds to go to completion. 8. For a reaction A+B → C, doubling the concentration of either A or B, quadruples the reaction rate. Write the rate law for the reaction.
14 of 15 The rate law for the reaction, A+B-C, that is zero order for both...
14 of 15 The rate law for the reaction, A+B-C, that is zero order for both reactants is O rate=k O rate=k[A] O rate=k[A][B] O rate=k[C] 15 of 15 For a reaction that is second order in A, calculate the value of the rate law constant using the table below: Experiment Initial [A]/M Initial rate/M s 0.010 0.020 .040 0 win 0.012 .050 0.19 3 0 118 M-18-1 O 126 M-15-1 O 0.40 M-15-1 O 121 M-15-1
1 of 15 All the following are true about reaction rates except A reaction rate can...
1 of 15 All the following are true about reaction rates except A reaction rate can be measured by change in concentration and time. Reaction rates can be estimated with the coefficients of the balanced reaction. Reaction rates change with temperature. Reaction rates change with the presence of a catalyst. 2 of 15 For the rate law, rate=k[A]?, determine k using the data table below: Initial rate/M s Experiment Initial [A]/M 1 0.15 0.30 2 3 0.0030 0.0120 0.0270 0.45...
12 of 15 Use the table below to calculate the initial reaction rate of the following...
12 of 15 Use the table below to calculate the initial reaction rate of the following reaction: 2AB+C [A]/M t/s 0.100 0.045 O 0.006 M/S -0.006 M/S -0.012 M/s 0.012 M/s 13 of 15 Use the table below to determine the rate law for the reaction A-2B: Initial rate/Ms Experiment Initial [A]/M 1 0.010 0.020 0.040 0.0010 0.0040 0.0160 2 3 1 rate=k O rate=k[A] O rate=k[A]2 O rate=k[A][B]2
1.Consider the following reaction: 4 NH + 5 O → 4 NO + 6 HO The rate of consumption of NH is -1.4...
1.Consider the following reaction: 4 NH + 5 O → 4 NO + 6 HO The rate of consumption of NH is -1.4×10 M/s. Calculate the rate of consumption of O. Use “E” for scientific notation. Do not enter units as part of your answer. 2.Consider the following reaction: 4 NH + 5 O → 4 NO + 6 HO The rate of consumption of NH is -1.4×10 M/s. Calculate the rate of production of HO. Use “E” for scientific...
lon 6 of 18 > Time (s) Determine the average rate of change of B from...
lon 6 of 18 > Time (s) Determine the average rate of change of B from 1 = Osto 1 = 232 s. 0 Concentration of A (M) 0.600 0.360 0.120 116 A2B 232 rates = 1.538 x10-3 я т т о т о Р F G H J K L
1. TL .lowing te deta was obtained experimentally. Rxn: A +28. 3 . D Rate (M/S)...
1. TL .lowing te deta was obtained experimentally. Rxn: A +28. 3 . D Rate (M/S) (M) [B] (M) C (M) 2.0 2056 0.050 0.20 2.0 0.050 0.10 0.20 50 0.25 0.10 0.20 16 0.050 0.40 a. Determine the rate law expression for this reaction (15 pts). Rate 4 = 0.40 = K [65[o oboJo no 2 - 8 Rate 2 0 .20 2 K[2[650[ 10 0.10 'b. What is the value for the rate constant (with proper units) (5...
DI Question 6 2 pts Consider the following Truth table 000 0| 0 000 11 00 10| 0 00 1 11 0100|1 01 0 11 0 01 1 0 | 0 01 1 1| 0 100 0 | 0 100 1| 1 10 1010 10 1 1| 1 11 001 O 11 0 1 1 0 Fill the followi...
DI Question 6 2 pts Consider the following Truth table 000 0| 0 000 11 00 10| 0 00 1 11 0100|1 01 0 11 0 01 1 0 | 0 01 1 1| 0 100 0 | 0 100 1| 1 10 1010 10 1 1| 1 11 001 O 11 0 1 1 0 Fill the following K-map 01 2 Select ▼ | [Select] 01 sect] | ▼ | [Select] ▼ | [Select] [Select] f11 15 | ▼...
Question 6 of 15 Submit A reaction has a rate law of Rate = (1.25 M-?s=')[A] [B]? What concentration of [B] would give the reaction a rate of 0.0891 if the concentration of [A] is 0.250 M?
thanks in advance ☺
(A). For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s (A), M [B, M (uncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 4 7.14 x 10-2 0.100 0.100 1.75 x 104 7.14 x 10-2 0.0500 0.200 1.76 x 104 3.57 x 10-2 0.0500 0.100 8.80 x 10-5 3.57 x 10-2 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction,...
7. Consider the following reaction A+B - products. The rate law was found to be Rate = k [A] [B]. Calculate k if [A] = 0.0500 M [B] = 0.125 M and the reaction took 405 seconds to go to completion. 8. For a reaction A+B → C, doubling the concentration of either A or B, quadruples the reaction rate. Write the rate law for the reaction.
14 of 15 The rate law for the reaction, A+B-C, that is zero order for both reactants is O rate=k O rate=k[A] O rate=k[A][B] O rate=k[C] 15 of 15 For a reaction that is second order in A, calculate the value of the rate law constant using the table below: Experiment Initial [A]/M Initial rate/M s 0.010 0.020 .040 0 win 0.012 .050 0.19 3 0 118 M-18-1 O 126 M-15-1 O 0.40 M-15-1 O 121 M-15-1
1 of 15 All the following are true about reaction rates except A reaction rate can be measured by change in concentration and time. Reaction rates can be estimated with the coefficients of the balanced reaction. Reaction rates change with temperature. Reaction rates change with the presence of a catalyst. 2 of 15 For the rate law, rate=k[A]?, determine k using the data table below: Initial rate/M s Experiment Initial [A]/M 1 0.15 0.30 2 3 0.0030 0.0120 0.0270 0.45...
12 of 15 Use the table below to calculate the initial reaction rate of the following reaction: 2AB+C [A]/M t/s 0.100 0.045 O 0.006 M/S -0.006 M/S -0.012 M/s 0.012 M/s 13 of 15 Use the table below to determine the rate law for the reaction A-2B: Initial rate/Ms Experiment Initial [A]/M 1 0.010 0.020 0.040 0.0010 0.0040 0.0160 2 3 1 rate=k O rate=k[A] O rate=k[A]2 O rate=k[A][B]2
lon 6 of 18 > Time (s) Determine the average rate of change of B from 1 = Osto 1 = 232 s. 0 Concentration of A (M) 0.600 0.360 0.120 116 A2B 232 rates = 1.538 x10-3 я т т о т о Р F G H J K L
1. TL .lowing te deta was obtained experimentally. Rxn: A +28. 3 . D Rate (M/S) (M) [B] (M) C (M) 2.0 2056 0.050 0.20 2.0 0.050 0.10 0.20 50 0.25 0.10 0.20 16 0.050 0.40 a. Determine the rate law expression for this reaction (15 pts). Rate 4 = 0.40 = K [65[o oboJo no 2 - 8 Rate 2 0 .20 2 K[2[650[ 10 0.10 'b. What is the value for the rate constant (with proper units) (5...
DI Question 6 2 pts Consider the following Truth table 000 0| 0 000 11 00 10| 0 00 1 11 0100|1 01 0 11 0 01 1 0 | 0 01 1 1| 0 100 0 | 0 100 1| 1 10 1010 10 1 1| 1 11 001 O 11 0 1 1 0 Fill the following K-map 01 2 Select ▼ | [Select] 01 sect] | ▼ | [Select] ▼ | [Select] [Select] f11 15 | ▼...
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