Spectrophotometry Post Lab

How can the reaction rate for a low pressure gaseous reactant be slow at high temperatures? Group of answer choices Particles may not have the correct orientation and/or low collision frequency. Particles may have low collision frequency and/or do not have enough surface area. Particles may not have the correct orientation and/or do not have enough energy. Particles may not have enough energy and/or low collision frequency. Particles may not have enough energy and/or do not have enough surface area. Particles may not have the correct orientation and/or do not have enough surface area.

Show ALL your steps, work and details in your calculations, use GRASPS: Given, Required, Analysis, Solution, and Paraphrase to answer the question, it is required. Answer in complete sentences and therefore statements.

What are limitations and improvements in this experiment and source of errors

Pre-lab questions 1. The stock concentration values cannot be used as the initial concentrations for the calculation of the reaction rate. Briefly explain. 2. Using these data, determine the order of reaction with respect to reactant A. A + B + C+ D Trial #1 Trial #2 Trial #3 [A], M [B], M 0.16 0.32 0.16 0.16 0.08 0.16 Rate, M/s 4.0x10* 8.0x10* 1.6x10* 3. Determine the order of reaction with respect to reactant B. 4. Calculate the rate constant for this reaction of A and B.

Answer 1 and 2. Show complete solution.

You continue with the Arrhenius Plot with the slope of the curve to be approximately -12,500 K and the Arrhenius factor of 4.367 E10 hours^-1. What is the shelf life of the drug at 22 C? What is the shelf life at 4 C? Be sure to show your calculations. Arrhenius Plot -8 -10 -12 -14 -16 -18 0.0026 0.0028 0.0030 0.0032 0.003 1/T In (k)

Name (please print): Fall 2022 Basic Laboratory Operations Post Lab Questions 1.) Suppose you're attempting to measure the density of a liquid that is highly volatile (it evaporates quickly). If you first measure the mass and then several minutes later you measure the volume of the liquid will the measured density be higher than the true value, lower than the true value, or the true density of the liquid. [It helps to understand this problem with the density equation.] 2.) Suppose you're attempting to measure the density of a liquid that is highly volatile (it evaporates quickly). If you first measure the volume and then several minutes later you measure the mass of the liquid will the measured density be higher than the true value, lower than the true value, or the true density of the liquid. [It helps to understand this problem with the density equation.] 3.) You're attempting to calculate the density of an alloy. The alloy is in the shape of a cylinder. If the mass of the alloy is…

Run Reactants Temperature (Celsius) Initial Rate (kPa/s)   1 10 ml 3% H2O2 = 5ml 0.5M KI 23.0 0.0798 2 5ml 3% H2O2 = 5ml 0.5 M KI 23.0 0.0391 3 5ml 3% H2O2 + 10ml 0.5 M KI 23.0 0.0794     Run Initial Rate (mol/L*s) [H2O2] after mixing [I-] after mixing 1 3.24 x 10^-5 0.147 M 0.0417 M 2 1.59 x 10^-5 0.0733 M 0.417 M 3 3.23 x 10^-5 0.0733 M 0.0833 M   Calculate the rate law for the reaction

I got #8a correct, but #8b is incorrect and I can’t figure out why? Please help.

3. The decomposition of N2O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO2 (g) + O2(g) The following results were collected: find nature) N2O5] 0.1000 Ln[N2O5] -2.30 2.65 2.99 -3.69 -4.38 -5.08 a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and Time (s) 10g. (LN) 0.0707 0.0500 50 0.0250 100 0.0125 200 0.00625 300 400 Ln[N2O5] versus time. Determine the value of k. Which graph did you use? graph *b. On your graph of [N2O5] versus time, highlight the times it takes for each halving of the reactant concentration. What is the half-life? Using this half-life calculate k. design experiments to find the activation energy,

21. The following data was obtained in a chemical kinetics experiment in which the concentration was measured every second. Determine the average rate of chemical consumption between 2 s and 6 s. Note: Show all calculations, follow the rules of significant figures, and box your final answer.

Nitric oxide gas (NO) reacts with chlorine gas according to the chemical equation given below. ½CI2 The following initial rates of reaction have been measured for the given NO +1 -> NOCI reagent concentrations. Experiment Rate (M/hr) [NO] (M) [Cl2] (M) 1 1.19 0.50 0.50 4.79 1.00 0.50 3. 9.59 1.00 1.00 What is the rate law for this reaction? 2.

Explain how changing Experimental Volume impacted the kinetics of the reaction. Compare to your prediction. Be concise. ( in short sentence)

Chemistry    Dear tutor dont copy from chatgpt if you do you will be reported    Using the internet , research the following terms as they relate to chemical reactions:   collision theory  Be very detailed    add graphs if needed  potential energy diagrams   be very detailed step by step  add graphs if needed  activation energy  be very detailed  add graphs if needed    Your work should be written in complete sentences, and assume your audience is grade 11 chemistry students who do not understand this unit. Make sure all research is put into your own words!

Introduction to Integrated Rate Laws Learning Goal: To understand how to use integrated rate laws to solve for concentration. A car starts at mile marker 145 on a highway and drives at 55 mi/hr in the direction of decreasing marker numbers. What mile marker will the car reach after 2 hours? This problem can easily be solved by calculating how far the car travels and subtracting that distance from the starting marker of 145. 55 mi/hr x 2 hr = 110 miles traveled milemarker 145 -110 miles milemarker 35 If we were to write a formula for this calculation, we might express it as follows: milemarkero- (speed x time) milemarker where milemarker is the current milemarker and milemarker, is the initial milemarker. Similarly, the integrated rate law for a zero-order reaction is expressed as follows: [A]orate x time [A] or since rate k[A] = k Azero-order reaction (Figure 1)proceeds uniformly over time. In other words, the rate does not change as the reactant concentration changes. In contrast,…

what is m and n

Can you please answer the second question on the handout that is attached thank you

You are trying to determine the KM for an enzyme. Due to a lab mishap, you have only two usable data points: Use these data to calculate an approximate value for KM. Is this value likely to be an overestimate or an underestimate of the true value? Explain.

Dinitrogen pentoxide rapidly decomposes in the atmosphere with the rate law noted. 2 N₂O5 (g) → 4 NO2 (g) + O₂(g) rate= (5.85 × 10-³s-¹) [N₂05] S How long does it take for sample to decompose from an initial concentration of 0.750M to0.211M ? Answer formatting tip: enter the reaction time using three significant figures; omit the units of s.

These questions are based on a reaction rate lab for my Chemistry homework. I attached my data values that I have already calculated. I think I am supposed to show more work for 4 and 5. I am genuinely confused on how to plot the graph too (6-7). Lastly, I am not sure if I got 8-10 correct? I think the rate law might be Rate = k [HCl] [Na2S2O3] but I am not sure if it needs an exponent or not?

I need to find the rate law to fill in the chart shown. Table 1-Initial moles The concentrations for all three stock solutions are given at the top of the data sheet. The volumes used for each experiment are in chart 1 on the data sheet.   Convert the volumes from mL to L using the metric system. Multiply the volume (L) by the molarity to determine the initial number of moles for each substance.

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