Be sure to answer all parts. Consider the reaction X + Y Z Initial Rate of...
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...
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
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
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...
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...
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 reaction X + Y rightarrow Z. 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 0.50 M and of Y is 0.040 M.
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?...
Using the following data, determine the rate law and calculate k: rate = k[F2]x[ClO2]y Experiment [F2] (M) [ClO2] (M) Initial rate (M/s) 1 0.40 0.05 1.2 M/s 2 0.20 0.10 0.60 M/s 3 0.40 0.10 2.4 M/s
2NO(g) + Br2(g) = 2NOBr(g) Experiment [NO-] (M) [Br2] (M) Initial Rate (M s-1) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 1.) Determine the rate law equation for the reaction. 2.) What is the overall order of the reaction? 3.) What are the value and the units of the rate constant, k? 4.) Write the expression to show how is the rate of disappearance of bromine, Br2, related to the rate...