CHM 101L M5 Factors Affecting Reaction Rates Lab Report

Table 2:  Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20     Please help me with this part, and please show me all steps  Order with respect to H2O2: Order with respect to KI:

question 1/2

Having a hard time with how to determine reaction rate

Answer question 3

60 50 40 kcal/mol 30 20 10 0 course of rx No activation energy is required OA. True OB. False •

Using the graph below, determine the time it will take for half of the reagent present at t = 60 sec to react. b.  196 s c.  256 s d.  120 s e.  60 s

1. This question is adapted from Harris 19-D. Carnosine is a dipeptide whose antioxidant properties protect cells from free radicals. Carnosine was determined by derivatization with naphthalene-2,3-dicarboxyaldehyde and cyanide followed by fluorescence detection using excitation at 445 nm and emission at 490. Quantification was by standard addition. To four aliquots of 20-ul cell lysate were added volumes of 100µM carnosine standard to generate final concentrations of 0, 1.0, 2.5, and 5.0 µM added carnosine. Solutions were diluted to 70µl before addition of 15µl of 5 mM naphthalene-2,3-dicarboxyaldehyde and 15µl of 10 mM NaCN. H H2N. OH Carnosine HN. Naphthalene-2,3- dicarboxyaldehyde Cyanide OH Fluorescent product HN. Fluorescence intensity Concentration (uM) of added carnosine in final 100 µL 0.0 0.465 1.0 0.698 2.5 1.029 5.0 1.651

A learning.mheducation.com Types of Reactions assignment and quiz F. Question Mode: Multiple Select Question Explain the different types of chemical react... https://moodle.coastal.edu/pluginfile.php/106... https://moodle.coastal.edu/pluginfile.php/106... Exit Assignment X Mc Graw Hill 13 of 36 Concepts completed i Multiple Select Question Select all that apply LI Which of the following reactions are expected to occur as written, with Ba reference to the activity series for metals (shown)? Select all that apply. Ca O Cu (s) + 2HCI (aq) → CuCl2 (aq) + H2 (g) Na Mg Mg (s) + Co(NO3)2 (aq) → Co (s) + Mg(NO3)2 (aq) Al Mn O Pb (s) + 2HCI (aq) → PbCl2 (s) + H2 (g) Zn Cr O 3Ag (s) + Fe(NO3)3 (aq) → 3ÄGNO3 (aq) + Fe (s) Fe NI Sn Pb H2 Cu Hg Ag Au Copyright O McGraw-Hll Education EText Alternative Need help? Review these concept resources. E Reading Rate your confidence to submit your answer. High Medium Low O2021 McGraw-Hill Education. All Rights Reserved. Privacy Terms of Use 80 888 DII DD F10…

A+B+CD Exp. Initial A (mol/dm³) Initial B (mol/dm³) Init. Rate of Formation of D (mol/dm³ min-¹) 1 0.10 0.10 3.0 x 10-4 2 0.30 0.30 9.0 x 10-4 3 0.10 0.30 3.0 x 10-4 4 0.20 0.40 6.0 x 10-4 5 0.10 0.10 1.2 x 10-3 The student concluded that the rate equation should be: rate = K[A] [B][C]² ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate equation, making sure that you include the correct units. Initial C (mol/dm³) 0.10 0.10 0.10 0.10 0.20

4

Experiment Initial Initial Initial rate/ concentration concentration mol dm-3 s-1 of A/mol dm-3 of B/mol dm-3 1 0.16 0.20 5.0 x 10-5 2 0.24 0.20 7.5 × 10-5 3 0.32 0.10 10.0 x 10-5 4 0.12 0.16 Determine value of X. Select one: O a. 2.50 x 10-5 O b. 3.00 x 10-5 О с. 3.75 х 10-5 O d. 4.00 x 10-5

Please help on whether I started the first problem correctly and if possible help on how to start the second question.

Answer both questions at bottom

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.

Help me fill out the rest please.

the mean time, the rate, [S₂O3] in the reaction may label clear outliers the mean) as such and e calculation. on mixtures NH4)2SO4 (NH4)2S2O8| (mL) (mL) 1.50 0.50 1.50 0.50 1.00 1.00 1.00 1.00 following reagents are um iodide ium persulfate m thiosulfate um nitrate ium sulfate odide in the solution in the Answer: 0.050 M • Determination of the rate law follows the protocol in ref. (5). with one difference. A reactant order (rate law exponent) will be calculated twice using two different pairs of determinations (e.g. determinations 1 & 2 and determinations 3 & 4). Then the mean is taken of both values and reported as order. This is done for each reactant. This additional step allows us to include more data and reduce experimental error. Practice Problem 2: The rate of a reaction CO(g) +3H₂(g)→ CH4(g) + H₂O(g) was determined at 25 °C. From the following data, determine a) the mean reaction order with respect to CO b) the mean reaction order with respect to H₂ c) the overall rate order d)…

Table 2:  Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20   Rate constant value                         Trial 1 ______________                         Trial 2 ______________                         Trial 3 ______________                         Average _____________

PLS HELP ASAP ON ALL ASKED QUESTIONS AND SHOW ALL WORK

Can you please complete and check if the answers are correct!!! Thank you in advance!!

Calculation Tables Table 4- Logarithms [l]o (M) -log[I]o -log(rate) [H2O2]o (M) 0.0100 -log[H2O2]o 2.00 Experiment # Rate (M/s) 1 2.63 x10-6 5.58 0.0200 1.70 5.18 x 106 0.0100 0.0400 0.0600 8.01 x 10-6 1.62 x 105 0.0100 4 0.0200 0.0600 3.21 x 105 0.0400 0.0600 Table 5- Rate Constants Experiment [H2OzJo(M) [H2O2]om Initial rate k # (M/s) 2.63 x10-6 1 0.0100 0.0200 2 0.0100 0.0400 5.18 x 10-6 0.0100 0.0600 8.01 x 106 4 0.0200 0.0600 1.62 x 105 5 0.0400 0.0600 3.21 x 105 Value of m (2 significant figures): Value of n (2 significant figures): verage value of k (3 significant figures):

Fast pls solve this question correctly in 5 min pls I will give u like for sure

X app.101edu.co # 3 E UL Week 7: Panopto DII 0 F3 $ R F4 X UL LTU 7-1A Identify the best conditions to complete the SN2 reaction shown below. H % 5 T N3 گیا QL FS A 6 Y Question 18 of 24 40 X F6 & 7 C|Chegg.com U F7 8 A) CH3I, THF B) NaCN, DMSO C) NaN3, ethylamine D) KI, THF X + E) NaN3, DMF PrtScn FB Home ( 9 F9 O ) End 0 & 3 ENG F10 P PgUp - F11 Tp S <10) 1 PgDn D + 6:16 PM 10/18/2022 F12

Question attached as photo.  This is not a exam/ test question:) you can see that our prof has written sth on this question, it is a question that he wants us to practice on our own in lecture. Thanks Topic related to 1st order/ 2nd order kinetics, need excel/graph to do this question, need TWO plots to check whether they are 1st/2nd order concentration = activity * m (concentration is proportional to activity plus a constant m) 1/[A] =1/[A]0 + Kt 1/[Activity* m] = 1/[Activity0 *m] +Kt 1/[Activity] =1/ [Activity]0 + mKt Do we follow the equations of zeroth, 1st, 2nd order reactions?  What is the key idea to determine whether this data gives 1st or 2nd order kinetics? Our prof was saying that if it's linear graph, means it is in correct order. BUT i have plotted 3 datas, two of them looks kinda linear to me. (the 2nd order and zeroth order graph are similar) If we are choosing from zeroth/2nd order, how do we determine its order if it's line is similar in linearity?

Construct the expression for Kc for the following reaction. HF(aq) = H*(aq) + F-(aq) 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. Kc 5 RESET [HF] 2[HF] [HF] [H'] 2[H*] [HF F1 2[F] [FF ||

For the arrhenius equation what are the other deviations for the formula like the ones i have to solve for t1 and k1.