chemical reaction rates:
1) Choose the option below that shows the equation that relates the rate of consumption of H+ and the rate of formation of Br2 for the given reaction.
5Brâ(aq)+BrOâ3(aq)+6H+(aq)â3Br2(aq)+3H2O(l)
Answers
6Î[H+]Ît=3Î[Br2]Ît
â16Î[H+]Ît=13Î[Br2]Ît
16Î[H+]Ît=13Î[Br2]Ît
â6Î[H+]Ît=3Î[Br2]Ît
Derive Rate Expressions for Relative
2) Consider the following reaction:
4NH3+7O2â¶4NO2+6H2O
If the instantaneous rate of reaction for ammonia was determined to be 6.4Ã10â2mole/L/s at 220 s, what is the instantaneous rate of reaction for the production of water?
Answers
6.4Ã10â2 mole/L/s
3.7Ã10â2 mole/L/s
9.6Ã10â2 mole/L/s
4.3Ã10â2 mole/L/s
chemical reaction rates:
1) Choose the option below that shows the equation that relates the rate of consumption of H+ and the rate of formation of Br2 for the given reaction.
5Brâ(aq)+BrOâ3(aq)+6H+(aq)â3Br2(aq)+3H2O(l)
Answers
6Î[H+]Ît=3Î[Br2]Ît
â16Î[H+]Ît=13Î[Br2]Ît
16Î[H+]Ît=13Î[Br2]Ît
â6Î[H+]Ît=3Î[Br2]Ît
Derive Rate Expressions for Relative
2) Consider the following reaction:
4NH3+7O2â¶4NO2+6H2O
If the instantaneous rate of reaction for ammonia was determined to be 6.4Ã10â2mole/L/s at 220 s, what is the instantaneous rate of reaction for the production of water?
Answers
6.4Ã10â2 mole/L/s
3.7Ã10â2 mole/L/s
9.6Ã10â2 mole/L/s
4.3Ã10â2 mole/L/s
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Related questions
Consider the reaction
2H3PO4âP2O5+3H2O
Determine the average rate of decomposition of H3PO4 between 10.0 and 40.0s.
Time (s) | 0 | 10.0 | 20.0 | 30.0 | 40.0 | 50.0 |
[P2O5] (M) | 0 | 1.90Ã10â3 | 4.90Ã10â3 | 6.70Ã10â3 | 7.90Ã10â3 | 8.50Ã10â3 |
Part B
Consider the reaction
5Brâ(aq)+BrOâ3(aq)+6H+(aq)â3Br2(aq)+3H2O(l)
The average rate of consumption of Brâ is 2.06Ã10â4M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval?
The kinetics of the reaction below were studied. The volumes of 0.040 M KBrO3, 0.040 M KI,
0.00050 M Na2S2O3, 0.040 M KCl, H2O and a buffer solution employed in each trial are shown
in the table below. One drop of 1% aqueous starch solution was also added in each trial. The
buffer solution was a pH = 4.74 solution containing 0.50 M acetic acid and 0.50 M sodium acetate; Ka = 1.8 x 10â5 for acetic acid. Each trial was performed at 25â¦C. For each trial, the reaction mixture was initially colorless after combining all solutions; appearance of a blue solution color in the reaction mixture signaled that all of the thiosulfate ion initially present had reacted and marked the end of the timing period. The initial reaction rate for each trial was calculated from the change in molar concentration of thiosulfate ion from each trial; the equation for calculating Initial Rate is shown below, where Ît is the elapsed time between combining all solutions and appearance of the blue solution color. Each solution volume was measured to the nearest 0.1 mL. (ie 5 mL shown in the table is 5.0 mL.)
BrO3- (aq) + 6Iâ(aq) + 6H+(aq) â 3H2O(l) + Brâ(aq) + 3I2(aq)
Initial rate = - 13âS2O32-ât
Volume (mL) Used
Trial # | KBrO3 | KI | Na2S2O3 | KCl | H2O | Buffer | Initial Rate (M/s) |
1 | 10 | 10 | 5 | 0 | 0 | 15 | 5.0 x 10â6 |
2 | 5 | 10 | 5 | 5 | 0 | 15 | 2.5 x 10â6 |
3 | 10 | 5 | 5 | 5 | 0 | 15 | 2.5 x 10â6 |
4 | 10 | 10 | 2.5 | 0 | 2.5 | 15 | 5.0 x 10â6 |
a)Which pair of trials could be used to determine the order for Iâ? Justify your choice.
b)How would you determine the order for H+? Be as specific as possible.
c)What would be the value for the initial rate if 5 mL KBrO3 solution, 5 mL KI solution, 5 mL Na2S2O3 solution, 10 mL KCl solution, 15 mL pH = 4.74 buffer solution, and 1 drop of 1% starch solution were used?
d)Why do Trials 1 and 4 have the same initial rate?
e)What time was required for the color change to occur in Trial 1?
f)What was the purpose of adding 5 mL of 0.040 M KCl in Trial 2?
g)How would you experimentally verify that KCl does not cause the color change from colorless to blue? Be as specific as possible.