6 I− (aq) + BrO3 − (aq) + 6 H+ (aq) à 3 I2 (aq) + Br− (aq) + 3 H2O (l)
TRIAL 1:
[I-] = 2.0x10^-3
[BrO3-] = 8.0x10^-3
[H+] = 2.0x10^-2
Celcius = 21
Time = 200 seconds
Rate constant = ?
Rate = ?
TRIAL 2:
[I-] = 4.0x10^-3
[BrO3-] = 8.0x10^-3
[H+] = 2.0x10^-2
Celcius = 21
Time = 100 seconds
Rate constant = 3.3x10^-7
Rate = 25.78
TRIAL 3:
[I-] = 2.0x10^-3
[BrO3-] = 1.6x10^-2
[H+] = 2.0x10^-2
Celcius = 21
Time = 100 seconds
Rate constant = 3.3x10^-7
Rate = 25.78
Consider the reaction: 5 Br¯ (aq) + BrO3 ¯ (aq) + 6 H+ (aq) → 3 Br2 (l) + 3 H2O (l) The rate of the loss of BrO3 ¯ at a particular temperature is -8.45 x 10-3 M/s. a. Determine rate of loss of Br¯ . b. Determine the rate of loss of H+. ANSWER BOTH A AND B
Consider the reaction 5 Br− (aq) + BrO3− (aq) + 6 H+ (aq) → 3 Br2 (aq) + 3 H2O (l) The average rate of consumption of Br− is 1.94 M/s over the first two minutes. What is the average rate of consumption of H+ during the same time interval? Enter your answer numerically in units of M/s.
The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]^2. BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l) What is the order of reaction with respect to Br - ?
Consider the following reaction in aqueous solution: 5 Br−(aq) + BrO3−(aq) + 6 H+(aq) ---> 3 Br2(aq) + 3 H2O(l) i) The equation that relates the rate expressions for this reaction in terms of the disappearance of Br−, BrO3− and the formation of Br2 and H2O is (Choose the correct letter.): NOTE: { } is being used to represent the molar concentration. A. R = -1/5{ Δ Br - }/ Δ t = -1/1{ Δ BrO 3- }/ Δ t...
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...
In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3-, and bromide ion, Br-, according to the following chemical equation. 3 BrO- (aq) --> BrO3- (aq) + 2 Br- (aq) A plot of 1/[BrO-] vs. time is linear and the rate constant, k, is equal to 0.056 M-1s-1. If the initial concentration of BrO- is 0.80 M, how long will it take* the concentration of the BrO- ion to be 0.40 M? *enter your answer in seconds
Solution 3. Initial [S, 0,2-) =0.050 M; initial [T"]=0.10 M. Time experiment started Time (s) between Total moles of Aliquor no. appearances of color Cumulative times (8) $20,2-consumed 12.0 2.0x10-- 4.0x10 134 6.0x104 8.0x10 10.x10- 12x10- 12 14x10 3 6 Solution 4. Initial [3,0,?'1-0.10 M; initial [T"]=0.025 M. Time experiment started Aliquot no Time (s) between appearances of color 189 Cumulative times (8) 189 1 2 3 Total moles of 5,92-consumed 2.0x10-- 4.0x10+ 6.0x10 8.0x10- 10.x10+ 12x10- 14x10- 208 209...
1 7. The initial rate of the reaction: BrOz (aq) + 5 Br(aq) + 8 H+(aq) + 3 Brz(1) + H2O(1) Has been measured at the reactant concentrations shown (in mol/L) Experiment [Br03-] [Br] [H] Initial rate (mol/(L:s)) 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.10 0.20 0.10 1.6 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) what is the rate law expression and the rate constant k? [3] b) what...
In the reaction of dichromate ion and iodide ion: Cr2O72-(aq) + 14 H+(aq) + 6 I-(aq) ---> 2 Cr3+(aq) + 7 H2O(l)+ 3 I2 (s) the oxidizing agent is ? and the reducing agent is ?
Given the information below: Rate= k[CH3COCH3]m [I2]n (aq) Trial Acetone (mL) HCl (mL) I2 (mL) H2O (mL) Total Volume (mL) 1 10 10 10 20 50 2 20 10 10 10 50 3 10 10 20 10 50 4 10 20 10 10 50 Trial Avg. Time (sec) ∆[I2] (mol/L) Rate = -∆[I2]/time ([mol/L]/s) 1 46.5 -0.000236 5.08*10-6 2 30.5 -0.000236 7.74* 10-6 3 138 -0.000472 3.42*10-6 4 26.5 -0.000236 8.91*10-6 How would...