6. For the reaction 2A(g) + B(g) + 2C(g) → D(g) + E(g) the following data were collected at constant temperature. Determine the correct rate law for this reaction. All units are arbitrary. Trial Initial [A] Initial [B] Initial [C] Initial Rate 1 0.150 0.350 0.0217 0.225 0.320 0.150 0.350 0.0439 0.225 0.250 0.350 0.0362 0.225 0.150 0.600 0.01270 1234

6. For the reaction 2A(g) + B(g) + 2C(g) → D(g) + E(g) the following data were collected at constant temperature. Determine the correct rate law for this reaction. All units are arbitrary. Trial Initial [A] Initial [B] Initial [C] Initial Rate 1 0.150 0.350 0.0217 0.225 0.320 0.150 0.350 0.0439 0.225 0.250 0.350 0.0362 0.225 0.150 0.600 0.01270 1234

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the reaction A → products, concentration and time data were collected. Enter these data into the graphing tool to determine the reaction order. t Graphing Tool 0.0 25.0 50.0 73.0 [A] 3.40 2.28 1.53 1.02 In[A] 1.223775 0.824175 0.425268 0.019803 Clear All Data 1/[A] 0.294118 0.438596 0.653595 0.980392 [A] 3.4 2.822 2.244 1.666 1.088 0.51 [A] vs. t to 0 14.6 t (s) 0.0 25.0 50.0 75.0 In[A] vs. t 29.2 t 43.8 1/[A] vs. t 58.4 [A] (M) 3.40 2.28 1.53 1.02 73
For the following reaction Mechanism write the overall reaction and write the rate law. H3O++ I- → HI + H2O (fast) H2O2 + HI → H2O + HOI (fast) HOI + H3O++ I- →2H2O + I2 (slow) I2 + I- → I3-(fast)
The decomposition of nitrosyl bromide is followed 2 NOBr → 2 NO + Br2 Time (s) [NOBr] (M) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 Determine the average rate over the entire experiment.
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) | Rate (M/s) reaction and select the appropriate units. 0.250 0.260 0.0234 A + 2B → C + D 0.250 0.520 0.0234 3 0.500 0.260 0.0936 Units k = M.s-1 M-²s¬1 M-ls-1
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t [A] In[A] 1/[A] Add Row 10 total rows What is the reaction order? Calculate the concentration of A after 127 s. [A]]27s = M [V)
Consider the reaction: 2 Br2 + NO 2 NOB.. A study of this reaction was conducted at 298 K. What is the rate law? [ Br2] [NO] Rate(mol/Ls) 1.20 1.60 0.0324 2.40 1.60 0.0638 0.600 3.20 0.0642
Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Write 2-3 sentences to describe how you determined the rate law for the reaction.
Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.450 0.50 0.300 1.00 0.225 1.50 0.180 2.00 0.150 2.50 0.130 3.00 0.115 3.50 0.100 4.00 0.090
Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =
The concentration of A was monitored for the reaction A → P and the following data were obtained. What is the rate law, rate = k [A]x, for this reaction? [A] (M) Time (s) 0.0200 0 0.0169 100 0.0142 200 0.0120 300 0.0101 400 0.0086 500 0.0072 600 0.0061 700 Question 15 options: rate = 1.7 x 10–3 [A] rate = 2.3 x 10–3 [A]2 rate = 0 54 [A] rate = 1.3 x 10–3 [A] rate = 0 54 [A]2
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] 3.4 3.4 1.223775 0.294118 25 2.28 0.824175 0.438596 2.822 + 50 1.53 0.425268 0.653595 2.244 + 75 1.02 0.019803 0.980392 1.666 - 1.088 - 0.51 - 15 30 45 60 75 t y=-0.03156 x + 3.241000 2= 0.971 Add Row 10 total rows What is the reaction order? O 1 Calculate the concentration of A after 127 s. [A]127 s = M [V)
Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]