Given the data, determine the rate law expression for the reaction: 2A+B(2 subscript)+C --> A(2 subscript)B+BC
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Given the data, determine the rate law expression for the
reaction: 2A+B(2 subscript)+C --> A(2 subscript)B+BC...
a. Given these data for the reaction A + B → C, write the rate-law expression....
a. Given these data for the reaction A + B → C, write the rate-law expression. Use k for the rate constant.) b. What is the value, with units, for the specific rate constant? The specific rate constant- Initial Rate of Initial [A] Initial [B] Formation of C Expt. (M) (M.s-1) 0.30 0.30 0.60 0.20 0.40 0.80 4.0 x 10-5 1.6 x 10-4 2.6 x 10-3
Given the initial rate data for the reaction A+BC, determine the rate expression for the reaction....
Given the initial rate data for the reaction A+BC, determine the rate expression for the reaction. [A], M [B].M Initial rate, M/S 0.10 0.20 5.00 10.20 0.20 10.0 0.10 0.15 2.81 O rate=250[A][B] rate - 5.0[A][B] rate=250[A)? rate - 50.0[A] rate= 1250[A][B] The first-order reaction A --> B+C has a half-life of 3.00 minutes. The rate equation for this reaction is rate = 1.50 min-1[A] rate = 1.05 min [A] O rate = 4.34 min [A] rate = 0.405 min...
need help with #3 please QUESTION 3 Determine the rate-law expression for the reaction below at...
need help with #3 please
QUESTION 3 Determine the rate-law expression for the reaction below at the temperature at which the tabulated initial rate data were obtained, rate- A + 2B + 3C - Products Experiment Initial [A] 0.10 M Initial [B] 0.20 M Initial [C] 0.10 M 0.40 M 0.20 M 0.10 M Initial Rate of Loss of A 4.0 x 10-2 Mmin 4.0 x 10-2 M/min 1.0 x 10- M'min 16x 10- Mmin 0.20 M 0.25 M 0.40...
For the reaction of 2A ---> B + C, the following data are obtained for [A]...
For the reaction of 2A ---> B + C, the following data are obtained for [A] as a function of time time (min) [A] (mol L-1) 0 0.80 8 0.60 24 0.35 40 0.20 a). Determine the order and the rate law of the reaction. (Hint: Consider the integrated rate laws shown on the first page). b). Calculate the value of the rate constant k
Determine the rate law given for the following reaction given the initial rate data in the...
Determine the rate law given for the following reaction given the initial rate data in the table: 2A + 2BC+2D Experiment [A] (M) [B] (M) Initial rate (M/s) 0.0211 0.113 2.00 x 10-5 2 0.0422 0.113 8.00 x 10-5 3 0.0422 0.226 1.60 x 10 1 Rate = K[A] [B] Rate = K[A] [B] Rate - AllB12 Rate - [A] [B]
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq)...
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq) + 5 C103(aq) + 6 H+(ag) Experiment Mn04] 0.10 2 0.25 3 0.10 4 0.10 2 Mn2+ (aq) + 5 C104 (aq) + 3 H20 (1) [C103] [H] Initial Rate(M/s) 0.10 0.10 5.2 x 10-3 0.10 0.10 3.3 x 10-2 0.30 0.10 1.6 x 10-2 0.10 0.20 7.4 x 10-3
B) Determine the integrated rate law for this reaction. C) Calculate the half-life for this reaction....
B) Determine the integrated rate law for this reaction.
C) Calculate the half-life for this reaction.
D) How much time is required for the concentration of A to
decrease to 4.25x10^-3 M
A certain reaction has the following general form: At a particular temperature and Alo 3.40 × 10-2 M concentration versus time data were collected for this reaction, and a plot of ln A versus time resulted in a straight line with a slope value of -2.91 x 10-2...
For the following reaction: 2A + B → 2 C The rate law is determined to...
For the following reaction: 2A + B → 2 C The rate law is determined to be: rate = 0.4357 [A][B] What will be the initial rate (in M/s) if initial concentrations are: [A] = 0.500 M, [B] = 1.54 [M]
Seat # Ver. K J. Quest. 6 (9 pts). The following initial rates were obtained for the reaction -120 kJ Δ Η 2C 2A +B [B] (M) 0.30 0.60 [A] (M) 0.20 Rate (M/s) 0.127 0.40 1.02 0.254 0.509 0.60 0.20 0...
Seat # Ver. K J. Quest. 6 (9 pts). The following initial rates were obtained for the reaction -120 kJ Δ Η 2C 2A +B [B] (M) 0.30 0.60 [A] (M) 0.20 Rate (M/s) 0.127 0.40 1.02 0.254 0.509 0.60 0.20 0.40 0.30 a. Determine the rate law for the reaction. b. Calculate the rate when B 0.40 M and A 0.65 M. a. With the aid of the rate law, propose a plausible two-step mechanism for the reaction. Label...
2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g...
2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g) → 2C(9) on the basis of the following proposed mechanism ki ZA K-1 X + B K2 20 To what expression does the rate expression reduce if the second reaction is slow, the initial equilibrium established very rapidly. (8)
a. Given these data for the reaction A + B → C, write the rate-law expression. Use k for the rate constant.) b. What is the value, with units, for the specific rate constant? The specific rate constant- Initial Rate of Initial [A] Initial [B] Formation of C Expt. (M) (M.s-1) 0.30 0.30 0.60 0.20 0.40 0.80 4.0 x 10-5 1.6 x 10-4 2.6 x 10-3
Given the initial rate data for the reaction A+BC, determine the rate expression for the reaction. [A], M [B].M Initial rate, M/S 0.10 0.20 5.00 10.20 0.20 10.0 0.10 0.15 2.81 O rate=250[A][B] rate - 5.0[A][B] rate=250[A)? rate - 50.0[A] rate= 1250[A][B] The first-order reaction A --> B+C has a half-life of 3.00 minutes. The rate equation for this reaction is rate = 1.50 min-1[A] rate = 1.05 min [A] O rate = 4.34 min [A] rate = 0.405 min...
need help with #3 please
QUESTION 3 Determine the rate-law expression for the reaction below at the temperature at which the tabulated initial rate data were obtained, rate- A + 2B + 3C - Products Experiment Initial [A] 0.10 M Initial [B] 0.20 M Initial [C] 0.10 M 0.40 M 0.20 M 0.10 M Initial Rate of Loss of A 4.0 x 10-2 Mmin 4.0 x 10-2 M/min 1.0 x 10- M'min 16x 10- Mmin 0.20 M 0.25 M 0.40...
Determine the rate law given for the following reaction given the initial rate data in the table: 2A + 2BC+2D Experiment [A] (M) [B] (M) Initial rate (M/s) 0.0211 0.113 2.00 x 10-5 2 0.0422 0.113 8.00 x 10-5 3 0.0422 0.226 1.60 x 10 1 Rate = K[A] [B] Rate = K[A] [B] Rate - AllB12 Rate - [A] [B]
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq) + 5 C103(aq) + 6 H+(ag) Experiment Mn04] 0.10 2 0.25 3 0.10 4 0.10 2 Mn2+ (aq) + 5 C104 (aq) + 3 H20 (1) [C103] [H] Initial Rate(M/s) 0.10 0.10 5.2 x 10-3 0.10 0.10 3.3 x 10-2 0.30 0.10 1.6 x 10-2 0.10 0.20 7.4 x 10-3
B) Determine the integrated rate law for this reaction.
C) Calculate the half-life for this reaction.
D) How much time is required for the concentration of A to
decrease to 4.25x10^-3 M
A certain reaction has the following general form: At a particular temperature and Alo 3.40 × 10-2 M concentration versus time data were collected for this reaction, and a plot of ln A versus time resulted in a straight line with a slope value of -2.91 x 10-2...
Seat # Ver. K J. Quest. 6 (9 pts). The following initial rates were obtained for the reaction -120 kJ Δ Η 2C 2A +B [B] (M) 0.30 0.60 [A] (M) 0.20 Rate (M/s) 0.127 0.40 1.02 0.254 0.509 0.60 0.20 0.40 0.30 a. Determine the rate law for the reaction. b. Calculate the rate when B 0.40 M and A 0.65 M. a. With the aid of the rate law, propose a plausible two-step mechanism for the reaction. Label...
2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g) → 2C(9) on the basis of the following proposed mechanism ki ZA K-1 X + B K2 20 To what expression does the rate expression reduce if the second reaction is slow, the initial equilibrium established very rapidly. (8)
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