Lab 4 ECH 1Y Coffee Design-Final draft

The concentration of the car exhaust fume nitrous oxide, NO2, in the air near a busy road is a function of distance from the road. The concentration decays exponentially at a continuous rate of 2.54% per meter.¹ At what distance from the road is the concentration of NO₂ half what it is on the road? Round your answer to the nearest integer. At i meters from the road the concentration of NO2 in the air is half the concentration on the road. At what distance from the road is the concentration of NO₂ 10% of what it is on the road? At i meters from the road the concentration of NO₂ in the air is 10% of the concentration on the road.

For each reaction, identify the reactant as an acid , a base , or neither an acid or base : a. HCl + H 2 O → H 3 O + + C l - , HCl is a/an ................................ ............... acid base neither b. NaCl + H 2 O → Na + (aq) + Cl - (aq), NaCl is a/an ................................ . acid base neither c. NaOH (s) → Na + (aq) + OH - (aq), NaOH is a/an ................................ . acid base neithe

Resarch project ( le chatelier's principle ) Be sure to explain the Chemistry involved in this reaction or process and how this reaction relates to Technology, Society and/or the Environment. Some examples include: Haber-Bosch Process Blood Buffering Ocean Acidification add lots of pictures and details

Is my answer correct?

Using the reaction and data in the table below answer the following series of questions. CH3OH(aq) + HCl(aq) ----> CH3Cl(aq) + H2O(I) Reaction CH3OH conc. HCl conc. Initial Rate (M/s) 1 0.100 M 0.100 M 1.1 x 10-2  2 0.200 M 0.100 M 2.3 x 10-2 3 0.100 M 0.200 M 1.1 x 10-2 *conc = concentration a.  The reaction is                                order in regards to CH3OH. b.  The reaction is                              order in regards to HCl.

What is the concentration after 3 minutes has passed?  a.) 0.0702 b.) 0.0693 c.) 6.421E-4 d.) 0.0664

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

Consider the balanced chemical equation. Submit Request Answer H2O2 (aq) + 31 (aq) + 2H+(aq) → I3 (aq) + 2H2O(1) In the first 12.0 s of the reaction, the concentration of I drops from 1.000 M to 0.773 M . Part B You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Predict the rate of change in the concentration of I3 (AI3]/At). Express the rate to three significant figures and include the appropriate units. A[l; ]/At = Value Units

Help with the question on the right Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOH), M [R'OHJ, M (HAJ, M Initial Rate, M-min"' - R-C+ k2 R С—0—Н + HA A- 0.35 0.35 0.50 4.60 0.50 0.62 0.35 0.35 8.14 0.81 0.50 10.6 0.35 0.50 0.75 0–H 9.84 Group 1 0–H 0–H k3 Rate = k[RCOOH][R'OH] R-Ć+ A- R 0–H R—С—0—Н + Rate = k[RCOOH][R'OH][HA] k4 0–H R-ó+ A- Group 2 Rate = k[RCOOR']/{[RCOOH][R'OH]} H Rate = k[R'OH] 0–H Rate = k[RCOOH] k5 R- C-0–R' R-C-0–H + H,о + НА R-o+ A- Group 3 Step 2 or Step 3 O Step 1 or Step 2 Step 1 Step 3 Step 2 Step 1

Which of the following reactions are written correctly? O 2HSO4laq) + 2NAOH(aq)→ 2NaSOa(aq) + 2H2O(U) H2SO4(aq) + 2 NaOH(aq)→Na2SO4(aq) + 2H20(0 O 2HCI(aq) + K2OH(aq) → 2KCI(aq) + H2O()

For the following questions (c and d), assume that the concentration of the hydroxide ion was initially 1.00 M, 3.00 M and 5.00 M (after mixing) for Runs #1, #2 and #3, respectively. c. Produce a plot of the pseudo-rate constants, Ln(k') vs. Ln[OH-], Calculation #7 on pg. 7. Determine the order of the hydroxide ion (Attach the relevant spreadsheet and plot). Order of OH-:__ (express as an integer) d. Using the intercept from the plot produced in 2c, determine the value for the rate constant, as described in Calculation #8 on pg. 7 k: 0.2647 Show your work here: K = e-3.6317 = 0.2647 3. Using the analysis in Question #2, determine the rate of reaction of chloromethane with the hydroxide ion at 61 °C, given initial concentrations of [CH3Cl] = [OH-] = 0.45 M?

Construct the expression Kc for the following reaction. 2 P(s) + 5 Cl2(g)=2 PCI:(g) 1 Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. Ko 5 RESET [P] [CL] [PCI:] 2[P] 5[Ch] 2[PCI:] [PF [Cl]$ [PCI:]? 2[P]? 2[PCIs]?

10. What are the major differences between a reaction occurring in flask in the laboratory compared to a reaction occurring in a biological system?

A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]0[B]2, what is the new rate if the concentration of [A] is increased to 0.200 M?   It says the answer was 0.0200 but im not sure, could you check and give me a step by step solution?

3 / 3 100% + | 5. The following series of reactions show the catalyzed conversion of oxygen to ozone: ½ 0, (g) + NO (g) → NO, (g) 2 NO, (g) → NO (g) + O (g) 2 O, (g) + O (g) → 0, (g) -> a) Write the overall reaction. b) Is NO, or NO the catalyst for this reaction? Explain your answer. the following reaction: