2 N₂05(9)→ 4 NO₂(g) + O₂(g) sider the decomposition of dinitrogen pentoxide shown above. In order to determine the rate of this reaction, we can measure the concentration of N₂O5 at various time intervals throughout the ction. The data and graph of [N₂O5] verses time are shown below. 0 200 400 Time (3) 600 800 1000 1200 1400 1600 1800 2000 M/sec (C) Which of the following is true as the reaction proceeds to longer times? O Rate slows down because the concentration of reactant is smaller. O Rate speeds up because the concentration of reactants is smaller. The rate slows down because the concentration of reactants is larger. O Rate slows down because the concentration of product is larger. O Rate speeds up because the concentration of product is larger. [N₂O₂] (M) 1.00 0.88 0.78 0.69 0.61 0.54 0.48 0.43 0.38 0.34 0.30 75- 25 (A) What is the average rate of consumption of N₂O5 in the first 400 seconds? NOTE: The sign is important! M/sec (B) What is the average rate of consumption of N₂O5 between 600 and 1200 seconds? 500 1000 1500 2000 Time()

2 N₂05(9)→ 4 NO₂(g) + O₂(g) sider the decomposition of dinitrogen pentoxide shown above. In order to determine the rate of this reaction, we can measure the concentration of N₂O5 at various time intervals throughout the ction. The data and graph of [N₂O5] verses time are shown below. 0 200 400 Time (3) 600 800 1000 1200 1400 1600 1800 2000 M/sec (C) Which of the following is true as the reaction proceeds to longer times? O Rate slows down because the concentration of reactant is smaller. O Rate speeds up because the concentration of reactants is smaller. The rate slows down because the concentration of reactants is larger. O Rate slows down because the concentration of product is larger. O Rate speeds up because the concentration of product is larger. [N₂O₂] (M) 1.00 0.88 0.78 0.69 0.61 0.54 0.48 0.43 0.38 0.34 0.30 75- 25 (A) What is the average rate of consumption of N₂O5 in the first 400 seconds? NOTE: The sign is important! M/sec (B) What is the average rate of consumption of N₂O5 between 600 and 1200 seconds? 500 1000 1500 2000 Time()

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...

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Consider Following reaction: CH4(g) + 4 NO(g) → 2 N2(g) + CO2(g) + 2 H2O(g) The concentration of NO was 3.176M at t = 0.39 s and 0.947 M at t = 7.60 s. What is the rate of consumption of CH4 in M/s? Report your answer with four decimals. Enter numbers only; do not enter units.
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Nitrogen, N2, is reacting at a rate of 75.0 mM/min to produce NH3 in the following reactionN2(g) + 3 H2(g) → 2 NH3(g)What is the rate of change of H2 and what is the rate of change of NH3? Give your answer in mM/min. (Note: mM = millimol/L = 0.001 mol/L)
Given the following data, determine the rate constant (in M-2s-1) of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) [Cl2] (M) Rate (M/s) 3.4 x 104 8.5 x 105 3.4 x 104 Experiment [NO] (M) 1 0.0300 0.0100 0.0150 0.0100 3 0.0150 0.0400 Note: Answers must be numeric, not alphanumeric-42, not forty-two.
A. Consider the following proposed mechanism for the production of chlorine dixoide from chlorine and ozone. Draw a reaction coordinate diagram for this reaction. Label reactants, products, transition states, intermediates, and activation energy on your sketch. Assume the reaction is endothermic. NOTE: CI is chlorine, not Carbon lodide Overall: Cl₂ (g) + 203 (g) → 2 CIO₂ (g) + O₂ (g) Step 1: Cl₂ (g) → 2 Cl (g) fast Step 2: Cl (g) + Os (g) CIO₂ +O fast Step 3: O (g) + O3 (g) → 202 (g) fast Step 4: Cl (g) + O2 (g) → CIO2 (g) slow
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) [CH3CI] / mol L-1 Initial Rate / mol L-1 s-1 Trial [Cl2] / mol L-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the order of the reaction with respect to Cl2?
(#28) Reaction Rates and time. A decomposition reaction in the first order has a rate constant of 1.26 x 10-4/sec. If the initial concentration of the reactant is 0.644 M. how much time will it take before 20% of the reactant has decomposed? 28a) In blank #1, type-in the working formula to solve for the time required. Enter the algebraic formula as a one-line equation and without spaces in between characters. Use lowercase for all fonts. 28b) In blank #2, type in your answer for the time it will take for 20% f the reactant to decompose. The answer is in seconds but do not include the unit. Enter your answer as a whole number with four significant figures.
60 QUESTION 13 The following graphs can be used for the questions that follow: 00 B0 00 Seris 1 02 time(min) D2 -D4 y = -0.0358x + 0.1058 Liner (Serive t) -18 time(min) The decomposition reaction of NO 2 is important in atmospheric chemistry. The reaction 2NO 2(g) → 2NO(g) + O 2(g) is second order with respect to NO 2. How can the rate constant be determined? A plot of 1/[NO2] versus time will be linear with a slope of -k. A plot of 1/[NO2] versus time will be linear with a slope of k. A plot of [NO2] versus time will be linear with a slope of -k. A plot of In[NO2] versus time will be linear with a slope of -k. Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air DD F8 F3 F4 F5 F1 %23 24 2 4. 7.
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2:26 ◄ Bartleby Experiment Determine the rate law for the following reaction using the experimental data given below. 2NO+O₂ → 2NO2 1 2 3 O rate=k[NO][0₂] O rate=k[NO]²[0₂] O rate=k[NO]²[0₂]² O rate=k[NO]²[0₂]³ O rate=k[NO]¹[0₂]³ [NO] (M) 0.0503 0.0247 Photo 0.0503 [0₂] (M) 0.0202 0.0202 0.0609 Rate (M/s) 0.355 0.0888 1.07 Done (+)