How do I solve for this?
Use the data table below to determine the value of the rate law constant for the first order reaction:
Experiment | Initial [A]/M | Initial rate/M s-1 |
1 | 0.10 | 0.0004 |
2 | 0.20 | 0.0010 |
3 | 0.30 | 0.0018 |
How do I solve for this? Use the data table below to determine the value of...
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...
Four experiments were conducted to discover how the initial rate of consumption of BrO3- ions in the reaction BrO3-(aq) + 5Br-(aq) + 6H+(aq) à 3Br2(aq) + 3H2O(l) varies as the concentration of the reactants are changed. Use the data given below to determine the average rate constant and write the rate law for this reaction. Experiment [BrO3-] (M) [Br-] (M) [H+] (M) Initial rate (M/s) 1 0.10 0.10 0.10 0.0012 2 0.20 0.10 0.10 0.0024 3 0.10 0.30 0.10 0.0035...
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
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...
I understand a-c, but not d.
The answer is 8.4 M/s but I do not know how to find it.
Consider the gas-phase reaction between nitric oxide and bromine at 273 °C: 2 NO(g) + Brz(8) — 2 NOBr(8). The following data for the initial rate of appearance of NOBr were obtained: Experiment Initial Rate (M/s) 24 2 [NO](M) 0.10 0.25 0.10 0.35 [Br21(M) 0.20 0.20 0.50 0.50 150 60 735 (a) Determine the rate law. (b) Calculate the average...
From the data table determine the rate law for reactions 1-4
and calculate the value of k for each. Thanks
I-IV
BACKGROUND
INFORMATION
Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2
Concentration= 0.44 M
•Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M
•Calculation of I^- after mixing for parts I,II, IV= 0.10
M
•Calculation of Initial (mol/L-s)
Filled in Table
Now the solutions for Rate Order and Rate Constant are
needed
Reactants 8 ml 30% HO, 2...
An experiment was conducted to determine the rate law for the
reaction A2(g)+B(g)→A2B(g) . The table above shows the data
collected. Based on the data in the table, which statement is
correct?
Trial 1 [A2] 0.10 [B] 0.50 0.20 0.50 Nm + Initial rate (Ms-1) 2.5 10-4 5.0 x 10-4 5.0 x 10-5 1.0 x 10-4 0.30 0.05 1 0.30 0.10 An experiment was conducted to determine the rate law for the reaction A2(g) +B(g) → A2B(g). The table above...
Timer Notes Eva mitial rate data are listed in the table for the reaction: (aq) + NO2 (aq) + N) () + H2O (1) Experiment (NH4): [NO] Initial rate (M/s) 0.21 0.10 72 x 10 0.10 3.6 x 10 0.15 0.12 5.4 x 10 4.3 x 10 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate (NH ) 155 seconds after the start of the reaction. In this experiment, both reactants...
Initial rate data are listed in the table for the reaction:
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2 (g) + H20 (1) Experiment (NH4+]: [NO 2-1. Initial rate (M/s) 0.24 0.10 7.2 x 10-4 0.10 3.6 x 10-4 10.12 0.15 5.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate [NH4+] at...
Using the information collected in the table below, determine the order of reaction with respect to the concentration of each of the reactants in the reaction: 1 X2 (g) + 2Y (g) + 2 Z (g) → XY(g) + XZ (g) + YZ (g) Expt. 1 [X2] [Y] [Z] initial rate 0.0010 mol/L 0.10 mol/L 0.0010 mol/L 2.0 x 10-4 mol/(Ls) 0.0010 mol/L 0.10 mol/L 0.0030 mol/L 1.8 x 10-3 mol/(Ls) 0.0040 mol/L 0.10 mol/L 0.0030 mol/L 7.2 x 10-3...