Class Practice C152-02 Chapter 16 Practice 2 - Rate Law Consider a chemical reaction between compounds...
26. Questions 26-27 refer to the following information. The reaction of acetone and bromine can be acid catalyzed as shown in the above reaction. The following initial rates of the bromination of acetone using an acid catalyst were measured at various initial concentrations as recorded in the table below. Trial [CH, COCH] Br] [H'] Initial Rate (Ms) catalyst 0.30 0.30 0.30 0.40 0.40 0.0500.050 0.10 0.050 0.050 0.050 0.050 0.050 0.10 0.20 5.7 x10- 5.7 x10 1.2 x104 3.I x10...
6. Consider the reaction X + Y → Z Initial Rate of Disappearance of X (M/s) [X] (M) [Y] (M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 From the data in the table, obtained at 360 K, (a) determine the overall order of the reaction (b) determine the initial rate of disappearance of X when the concentration of X is 0.30 M and that of Y is 0.40 M. ________ M/s
Be sure to answer all parts. Consider the reaction X + Y Z Initial Rate of Disappearance of [X] (M) [Y](M) X (M/s) From the data in the table, obtained at 360 K, 0.053 0.10 0.50 (a) determine the overall order of the reaction 0.20 0.30 0.127 1.02 0.254 0.40 0.60 0.20 0.60 0.30 0.509 0.40 (b) determine the initial rate of disappearance of X when the concentration of X is 0.40 M and that of Y is 0.30 M....
Be sure to answer all parts Consider the reaction X + Y → Z Initial Rate of Disappearance of |[XI (M) [YI(M) X (M/s) From the data in the table, obtained at 360 K, 0.053 0.127 1.02 0.254 0.509 0.10 0.20 0.30 0.40 0.20 0.60 0.40 0.30 0.50 (a) determine the overall order of the reaction 0.60 (b) determine the initial rate of disappearance of X when the concentration of X is 0.30 M and that of Y is 0.50...
Consider the reactionX + Y→ ZFrom the following data, obtained at 360 K, (a)determine the order of the reaction, and (b)determine the initial rate of disappearance of X when the concentration of X is 0.30 M and that of Y is 0.40 M.Initial Rate of Disappearance of X (M/s)[X](M)[Y](M)0.0530.100.500.1270.200.301.020.400.600.2540.200.600.5090.400.30
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. What is the reaction order with respect to B? Also, how do you find the value of the rate constant k for this reaction? Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4
Consider the equation: 2A + B → C The initial rate of reaction is measured at several different concentrations of the reactants with the following results: [A] (M) [B] (M) Initial Rate (M/s) 0.40 0.10 0.026 0.10 0.10 0.026 0.40 0.20 0.103 (blank 1) What is the order with respect to reactant A? (write a number) (blank 2) What is the order with respect to B? (write a number) (blank 3) What is the value of the rate constant. Include...
solve. also which experiments do you use and why? + Y Z 5) Consider the following reaction and data: X Experiment [X]. (M) [Y](M) 0.10 0.50 0.20 0.30 0.40 0.60 0.20 0.60 0.40 0.30 Initial Rate (M/s) 5.3 x 102 1.27 x 10' 1.02 x 10[21-[2]'=8 2.54 x 10-4 5.09 x 10 a) What is significant about an initial rate? You know the initial concentrations, know there is no quilibrium inppening, r it is the fastest, (73) b) Determine the...
Consider the hypothetical reaction: 2 X + Y → Z and its general rate law Rate = k[X]m[Y]n The following data was obtained when the reaction studied at –10°C: [X], M [Y], M Rate, M/min 0.10 0.10 0.18 0.10 0.20 0.36 0.20 0.20 1.45 (a) What is the order of reaction with respect to X? (2 points) (b) What is the order of reaction with respect to Y? (2 points) (c) What is the overall order of reaction?...
5. The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S2O82−](M) . [I−](M) . Initial Rate [M/s] 1 0.0300 0.0840 8.80 × 10−4 2 0.0300 0.0420 4.40 × 10−4 3 0.0600 0.0420 8.80 × 10−4 (a) Which of the following equations represents the rate law for this reaction? What is the...