Instructions Complete the Post-lab for Lab 10 - Kinetics after completing the laboratory exercise. This post-lab is due before the beginning of the next lab meeting. Multiple Attempts Not allowed. This test can only be taken once. Force Completion This test can be saved and resumed later. Your answers are saved automatically. * Question Completion Status: Save and Submit L A Click Submit to complete this assessment. Question 10 Question 10 of 10 1 points Save Answer The lodine Clock Reaction where the solution turns blue-black at the end was the experiment performed three times in this lab to investigate the effect of concentration on rate of reaction. The experiment was then repeated for a fourth trial. The concentration of the H2O2 was decreased to 0.375 % and the concentration of Solution A kept the same as the three trials used in this lab experiment. The time of Trial 4 was 74.93 seconds from the moment the two solutions were mixed until the solution turned blue-black. Keeping in mind that the starting concentration of S2032 was still 0.030 M, calculate the average rate of consumption of S2032 in molarity per second (M/s) for Trial 4. Round off the rate to the proper degree of certainty. Record the rate for Trial 4 with the proper units in the answer space provided. A Click Submit to complete this assessment. H <

Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced and contains state symbols after every reactant and product. HNO, (aq) + H,0(1) - Check Explanation O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 80 F Cloudy DELL Delete PgUp Insert F12 F10 F11 F9 F7 F8 F5 F6 Hum F4 F2 F3 Loc Esc F1 Backspace & Fn # 7 8 5 %24

help  please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89

TABLE 4: FIND THE CHEMICAL EQUATION

Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 1.8 × 10-5 [500.0] [0.200] RESET [5.00] [1.0 × 10-9] [1.0 × 10-9] [1.8 × 10-5] [x + 5.00] [x + 1.0 × 10] [x-1.0 x 10 x + 1.0 × 10-] [x-1.0 × 10-] [x+1.8 × 10] [x-1.8 × 10%] [0] [x-5.00] < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression, Ka (Part 2), determine the original mass of solid CH3COONa added to create this buffer solution. MNACH3COO g 0 0.360 30 21 43 11 15 36 x 10' 59 x 105 43 x 105 RESET 59 50

please. helpp. this unit is about chemical kinetics. PLEASEE ANSWER BOTH AS THEY ARE PART OF 1 QUESTION ONLY. I REALLY NEED HELP