e net ionic reaction is; Zn(s) + 2H,O*(aq) → Zn²*(aq) + H,(g) drochloric acid is a strong acid and acetic acid is a weak acid. Based on the above information, explain th the two reaction rates.

For our reaction, the last reagent to be added to the reaction mixture is the Permanganate; step 6 of the procedure below. The timing of the reaction starts "when half of the Permanganate solution has been added to the test tube." This choice is arbitrary and could be problematic. Under what circumstances could it be problematic?

Write the concentration equilibrium constant expression for this reaction. 31,(s)+2 Cr"(aq)+7H,0(1)→Cr20; (aq)+61 (aq)+14H*(aq) 3+

How long will it take for the concentration of A to decrease from 0.850 M to 0.205 for the reaction A → Products? (k = 0.0882 M⁻¹s⁻¹)

1. Below are the data for the decomposition of P2O5.  t., minutes    [P2O5]      1.25 0.852 6.52 0.721 12.22 0.602 17.90 0.501   (a) Determine the value of k for the reaction (be sure to include units). (b) What will the concentration of [P2O5] be at 28.50 minutes?  (You will need to use the value of k and the integrated rate law.) (c)  How long must the reaction proceed until [P2O5] is 0.111 M?

The pH change during a reaction will be followed by inserting a pH probe into a relatively small volume of liquid sample,  At least 1.5 cm of the pH probe must be immersed in the reaction solution. What is the best choice of reaction vessel for this reaction?      a volumetric flask      a Berzelius beaker      a Griffin beaker      a round bottomed flask      an Erlenmeyer flask

How long will it take for the concentration of A to decrease from 0.850 M to 0.271 for the reaction A → Products? (k = 0.0882 M⁻¹s⁻¹)

Which of the reactions that do not occur can be made to occur if an acid catalyst is added to the reaction mixture?

THE ACTIVATION ENERGY OF THE REACTION BETWEEN PERSULFATE AND IODIDE IONS, During the reaction of the persulfate ion with the iodide ion, iodine is produced. The molar relationship between the persulfate ion and iodine is 1:1. Iodine turns the colour of starch indicator from colourless to blue. If we add starch indicator to the reagent solutions, we see a blue colour as soon as the reaction starts, and products are formed. If we want to measure a rate constant, we want to remove some of the iodine until, for example, one quarter of the persulfate has reacted. This we can achieve by adding a predetermined amount of thiosulfate to the reagent solutions, because thiosulfate reacts with iodine as follows to form iodide and tetrathionate: 2 S₂03² + 1₂ = 21 +S406 ² A certain amount, which we can calculate to be 1/4 of the initial persulfate concentration of the iodine is thus removed, and at the same time iodide is produced, so that the iodide ion concentration remains constant.…

At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time.                    [H202] (mol/L) 0.                           1.600 3.10*10^4              0.592 6.20*10^4.            0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production