IC_4603_L21_Reaction_Rates

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

What are relevant chemical concepts, ideas and theories of this experiment

Final Reactant Concentrations and Reaction Rates   [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258   2 0.0033 0.0666 0.0166 135   3 0.00166 0.0133 0.0166 132   4 0.00166 0.0066 0.033 78   FIND THE RATE?

Final Reactant Concentrations and Reaction Rates   [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258 1.08 x 10^-7 2 0.0033 0.0666 0.0166 135 2.07 x 10^-7 3 0.00166 0.0133 0.0166 132 2.12 x 10^-7 4 0.00166 0.0066 0.033 78 3.58 x 10^-7 1.Using the information above determine the rate law (m, n and p) for the reaction. Show all calculations/reasoning in your notebook.   m_______________ n_________________ p ____________

1. Determine the rate of each experiment: Reaction # Concentration, M Time, seconds Rate (M/s) 1 0.050 90 2 0.10 90 3 0.15 90 4 0.20 90

Use the reaction below and the table of data to answer Questions 1-5. 2 NO(g) + Br₂ (8) 2 NOBr (g) [NO] (M) 0.250 0.250 0.300 0.900 Experiment # 1 #2 #3 #4 Question 1 Based on the data in the table, what is the reaction order of NO? Question 2 [Br₂] (M) 0.400 0.800 0.500 0.500 Based on the data in the table, what is the reaction order of Br₂? Question 3 Based on the data in Experiment #3, what is the rate constant k? Question 4 How many sig. figs. should be reported for the rate constant k? Initial Rate (M/s) 0.110 0.440 0.206 0.618

Initial Rate of Reaction Based on Initial Concentration of Reactants Concentration of Concentration of Initial Rate Trial A (M) B (M) (M/s) 1 0.256 0.628 2.56 x 10-3 2 0.0512 1.056 1.02 x 10-3 3 0.256 1.584 6.46 x 10-3 4 0.1024 1.056 2.05 x 10-3 Based on the above information, what is the rate law for the below reaction? (Use "k" for the rate constant and ^ for the exponent.) 2 A + 2 B – → C +D

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.

When fitting data to a best fit line, a correlation coefficient (R2) is determined and used to evaluate the quality of fit. The best fit of the data will have an R² value closest or equal to zero (0). closest or equal to one (1). equal to the rate of the reaction occurring. equal to the rate constant of the reaction occurring.

Sample Designs: Test one group against another group of experiment on the same reaction time test Compare the reaction times of the same people under two different conditions, like after exercise A test subject attempts to grab the ruler as it is dropped, the number on the ruler where the fingers grasp it can be used to judge reaction time Digital reaction time tests are easy to find with a google search You can also install an app on your phone that can measure reaction time (useful if you want to test subjects outside of class) C) How will you gather data? Will you take averages?

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DATA: Data Table 1. Part 1: The Effect of Temperature on Reaction Rate Temperature, °c 0.8°C Reaction Time, s 67.5 s 6.9 °C (not shown in video) 12.3 °C (not shown in video) 40.1 s 21.4 s 20.1 °C 11.3 s 35.6°C 1.2 s

The following reaction was analyzed and data was collected. 3 A (g) + 2 B4 (g) + C2 (g) – D (g) Initial Concentration (mol L) (Ba] 0.100 Trial Initial Rate (mol Ls4) 9.072 x 109 3.629 x 10 2.449 X 107 3.135 х 10% [A] [C:] 1 0.100 0.400 2. 0.400 0.100 0.400 0.100 0.300 0.400 4 0.100 0.600 1.60 0.600 0.75 0.100 a) Determine the rate law and rate constant for the reaction. Be sure to show all of your work. b) Determine the rate for the fifth reaction.

Can someone help me solve this I'm completely lost

Consider the following reaction and the data given in the table. 21+2 Fe(CN)63 - 12 + 2 Fe(CN),4- Trial Concentration of I- (M) Concentration of Fe(CN)63- (M) Initial Rate (M/s) 1 0.010 0.010 1.0x10-5 2.0x10-5 8.0x10-5 2 0.020 0.010 0.020 0.020 4 0.040 0.030 ?? (a) Which trials do you select to find the order with respect to 1? (b) The order of the reaction with respect to l" is 3-? (c) Which trials do you select to find the order with respect to Fe(CN)6 3-is (d) The order of the reaction with respect to Fe(CN)6 (e) The overall order of the reaction is (f) The value of the rate constant is (g) The initial rate of the reaction for trial 4 is

How does temperature affect the rate of this chemical reaction.

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Plot a Graph and Determine the Rate: Make a graphical plot of reaction time (× axis) and average (y axis). Determine the initial velocity (rate of the reaction by extending the initial straight-line portion of your reaction curve and calculating the gradient of the straight line (difference in y/ difference in ×).  What is the reaction rate based on your plotted values

In the reaction scheme CH,CH, + HCI 7. OH (aq), reflux CH,CH,CI - CH,CH,OH Step I Step 1 The percentage conversion for steps 1l and 2 are respectively 72% and 25% The overall percentage conversion of CH,CH2 to CH,CH,OH is: A 18 B 97 47 48.5

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: 14 A Moving to another question will save this response. Question 1 Record your response as a numerical response only. Question 1 of 10 >>>> 1 points Save Answer In general, reaction rates double when the temperature is increased by 10° C. The temperature of a reaction is increased by 30° C. The rate of the reaction will increase by a factor of: A Moving to another question will save this response. Question 1 of 10 >>>> K

1. Factors Affecting Reaction rate 1A. Effect of Reactant Concentration Test Concentration Observation Initial Final Total Tube # of HCI Time Time Time Slow evolution of colorless gas, Fast evolution of colorless 0 sec O sec 17 min 1 1.0 M 5 sec 4 min 2.0 M 38 sec gas Very fast evolution of colorless gas O sec 1 min 20 sec 3 3.0 М 2.

Please help me, double and triple check your answers. there are 2 parts attached as 2 screenshots