I'm guessing m is the reaction order for acetone. The reaction rate is given (in this case) by:
If we consider the times for reaction 1 and 2, we can see that for reaction 1 the time is exactly half than for reaction 2, which means that the rate of reaction 1 is double the rate of reaction 2.
We can calculate the concentration of acetone in both cases using the dilution formula:
Where 1 and 2 refer to values before and after dilution.
We use this and calculate:
Since the volumes of the other reactants and the final volume is the same in both reactions, we know that their concentrations don't change. We can take advantage of this to propose:
We know that the rate in 1 is double the rate in 2, so: V1 = 2 V2. Our expression is now:
So, we have:
Which means that m = 1.
4. Using the following information, calculate m. 4 M Acetone 1.0 M HCI 0.005 MI, 10...
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3. A third reaction mixture was made up in the following way: 5 mL. 4.0 M acetone+ 5 mL 0.0050 M12+ 10 mL 1.0M HCI+5 mL H2O a. What were the initial concentrations of acetone, 12 and H' ion in the reaction mixture? b. It took 109 seconds for the 12 color to disappear from the reaction mixture when at the same temperature as in question 1. What was the rate...
A) in a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 10 mL 4.0 M acetone + 10 mL 1.0 M HCl + 10 mL 0.0050 M I2 + 20 mL H2O What is the total volume of the sample? V = ___ mL B) In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 10 mL 4.0 M acetone + 10...
Determination of the Rate Law for the Iodination of Acetone in
Acidic Solution
I conducted an experiment to determine initial concentrations of
reactants, reaction times, and reaction orders for the iodination
of acetone.... here is my data followed by some questions... help
please??
1. How do you double the concentration of one of the reactant
solutions in each experiment? What reagent should you use to
control the total volume of each experiment?
2. Could you reduce the concentration of a...
3. (30 pts. total) We discussed the iodination of acetone in class. An alternative, but equivalent, way of writing the reaction is: acid H3C-C-CH3 + 131 acetone triiodide H3C-C-CH2 + 21 + H* iodoacetone iodide Is provides a more useful way to introduce 12 into the system. Iz is also useful because it absorbs visible light, and the rate of the reaction can be monitored by measuring the decrease in its absorbance at 565 nm. (Any time you can measure...
Calculate the pH of the following solutions at 25 ℃ a) 1.0×10-5 M HCI c) 1.0×10-5 M NaOH Number Number pH b) 0.01 M HNO, d) 0.1 M KOH Number Numbero pH-
co 4. A fourth reaction mixture was made up in the following way: ?? mL 4.0 M acetone + 10 mL 0.0050 M 12+5 mL 1.0 M HCI + ?? mL H2O a. If the reaction is zero order in Iz then what volumes of acetone and water are needed in order to (1) double the iodine concentration compared to reaction one and (2) then proceed at the same rate as in reaction 1 (note that the concentration of iodine...
Lab 20A lodination of Acetone Concentration SJBoylan2018 RATIO METHOD TO DETERMINE REACTION RATE MODEL You add 10 mL of 4.0 M acetone, 10 mL of 1M hydrochloric acid and 20 mL of water to a 125 mL Erlenmeyer ask. You mix the solution. Then you add 10 mL of 0.0050 M iodine to the flask, mix the solution and start a timer. At time equals zero the color of the solution is straw yellow with a hint of orange. This...
4. A second reaction mixture (Mixture II) was made up in the following way 20.0 mL. 4.0 M acetone + 10.0 mL 1.0 M HCI + 10.0 mL 0.0050 M 12 + 10.0 mL H20 What are the new initial concentrations of acetone, H' ion, and I2 in this second reaction mixture? Show your work! a. [acetone] M; [H'] M; [12] M It took 125 seconds for the l2 color to disappear from the reaction mixture when it occurred at...
Given the following reaction mixtures and the reaction: CH3COCH3 + Br2 -- > CH3COCH2Br + H+ + Br- Reaction Mixture Temperature º C Water (ml) 4 M Acetone 1 M Hydrochloric Acid 0.005 M Br2 1 25 20 10 10 10 2 25 10 20 10 10 3 25 25 10 10 5 4 25 10 10 20 10 The following reaction measurements were made: Reaction Mixture Times (s) 1 116 2 58 3 118 4 232 Calculate the reaction...
f) (6 pts) Which of the following mixtures will make a buffer? (Circle only one!) r? Circle onlyone f)(6 1000 mL fh following mix oc m will make a b S a) 100 mL of 1.0 M HCI +100 mL of 1.0 M NaOH +100 mL of 0.50 M HF 100 mL of 1.0 M HCI c)100 mL of 1.0 M HF +100 mL of 0.50 M NaOH 100 mL of 1.0 M HF +100 mL of 1.0 M NaOH...