ExperimentInitial [HgCl,]Initial [C,O,²-]Initial Rate of Formation of Cl-(M/min)0.52x10-4(1)(2)(3)(4)0.0836 M0.0836 M0.202M0.404M2.08 x 10-40.0418 M0.0316 M0.404M1.06 x 10-4?1.27 x 104d. Calculate the rate constant. Specify units.e. Calculate the initial oxalate ion concentration for Experiment 4.f. Calculate the rate of the formation of Cl- if (HgCl;] = 0.030 M and [C,O,'] = 0.060 M?

Initial [HgCl,] Initial [C,O,² ] Initial Rate of Formation of Cl- (M/min) 0.52x10 2.08 x 104 1.06 x 104 Experiment 0.0836 M (1) (2) (3) (4) 0.202M 0.404M 0.0836 M 0.0418 M 0.404M 0.0316 M 1.27 x 10 d. Calculate the rate constant. Specify units. e. Calculate the initial oxalate ion concentration for Experiment 4. f. Calculate the rate of the formation of Cl- if [HgCl,] = 0.030 M and [C,O, ] = 0.060 M?

Initial [HgCl,] Initial [C,O,² ] Initial Rate of Formation of Cl- (M/min) 0.52x10 2.08 x 104 1.06 x 104 Experiment 0.0836 M (1) (2) (3) (4) 0.202M 0.404M 0.0836 M 0.0418 M 0.404M 0.0316 M 1.27 x 10 d. Calculate the rate constant. Specify units. e. Calculate the initial oxalate ion concentration for Experiment 4. f. Calculate the rate of the formation of Cl- if [HgCl,] = 0.030 M and [C,O, ] = 0.060 M?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...

See similar textbooks

Similar questions

Table 2:  Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 2 3 Order with respect to H2O2 ___________________ Order with respect to KI ______________________
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Order with respect to H2O2: -0.138 Order with respect to KI: -0.828 Rate constant value                         Trial 1: 5.84                         Trial 2: 5.55                         Trial 3: 5.56                         Average: 5.6 -Please help me with this part, please 1. Should the rate constant (k) be the same for all three trials in this experiment? Explain your answer. 2.Write the complete rate law for this reaction.
Given the following data, determine the rate law and calculate K               Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4 the units on K are M-2s-1. You should enter the answer without units to 2 sig figs.
Given the following data, determine the rate law and calculate K Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4 the units on K are M-2s-1. You should enter the answer without units to 2 sig figs. Enter only the numerical value of K
Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.310 0.370 0.0139 2 0.310 0.740 0.0139 3 0.620 0.370 0.0556 Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D ?= Units:
Consider the reaction A+2B⇌CA+2B⇌C whose rate at 25 ∘C∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A][A](MM) [B][B](MM) Rate(M/sM/s) 1 0.20 0.010 4.8×10−4 2 0.20 0.020 9.6×10−4 3 0.40 0.010 1.9×10−3 Calculate the initial rate for the formation of CC at 25 ∘C∘C, if [A]=0.50M[A]=0.50M and [B]=0.075M[B]=0.075M. Express your answer numerically in molar per second using two significant figures.
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Rate constant value Trial 1 ______________ Trial 2 ______________ Trial 3 ______________ Average _____________
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
The following results were found after completion of Part C in the Experimental procedure: 0.056 M I- and 0.048 M H2O2 were used Run Catalyst Calculated Rate of Reaction (M/s) 1 none 0.031 2 10.00mL of 0.35 M FeCl2 0.52 Assuming the Rate Law = k[I-][H2O2] 2 Calculate the value of k for run 2. Give your answer to the nearest whole number.
Examine the experimental data shown in the table below for the following reaction: (make sure to show your work for each part) A + 5B + 6C ---> 3D + 3E Experiment [A] (M) [B] (M) [C] (M) Rate (M/s) 1 0.35 0.35 0.35 8.0 x 10-4 2 0.70 0.35 0.35 3.2 x 10-3 3 0.70 0.70 0.35 6.4 x 10-3 4 0.70 0.35 0.70 3.2 x 10-3 A. What is the reaction order of A? B. What is the reaction order of B? C. What is the overall rate equation for this reaction? D. What is the value of the rate constant? E. What are the units of the rate constant?
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
Rate Law find the initial rate N2O4 - 2 NO2 experiment initial (N2O4) (M) initial rate (M/sec) 1 0.50 0.050 2 1.00 0.200 3 1.50 0.450