Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![Consider the reaction, A--> Products, whose rate law is zero-order. Which of the
following graphs will produce a straight line?
A Plot of [1/[A]. vs time
B Plot of [A] vs time
C Plot of In[A] vs time
D Plot of [A] vs 1/time
O A
OB
O C
D.](https://content.bartleby.com/qna-images/question/cdbd63e3-7abd-454a-8818-4cd3e73b461b/6fb0731f-5761-4ab0-b80e-2294fd8b6df5/86zbcq_processed.jpeg)
Transcribed Image Text:Consider the reaction, A--> Products, whose rate law is zero-order. Which of the
following graphs will produce a straight line?
A Plot of [1/[A]. vs time
B Plot of [A] vs time
C Plot of In[A] vs time
D Plot of [A] vs 1/time
O A
OB
O C
D.
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- O KINETICS AND EQUILIBRIUM Using reactant reaction order to predict changes in initial rate A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of signifícant digits. [H] ['N] H, initial rate of reaction 1.51 M 1.34 M 4. 6.00 x 10 Mis 2.63 M | Mls 1.34 M 6.70 M 0.302 M Mis Explanation Check O 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility www rew IIarrow_forward5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.arrow_forwardFor a reaction with the rate law below: Rate = k[A]? %3D a plot of In[A] vs. time gives a straight line. a plot of 1/[A] vs. time gives a straight line. a plot of 1/[A] vs. 1/time gives a straight line. O a plot of [A] vs. time gives a straight line. O a plot of log [A]o/[A] vs. 1/time gives a straight line. A Moving to another question will save this response. esc 20 F3 F1 F4 $4 1. 2. 4 Q W R. # 3arrow_forward
- A certain reaction is second order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N-] initial rate of reaction 0.153 M 1.80 M 13.0 M/s x 5 ? 0.245 M 1.80 M O MIs 0.618 M 0.445 M M/sarrow_forwardUnits of M s-1 pleasearrow_forwardA certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H,] initial rate of reaction x10 2.37 M 0.112 M 0.123 M/s alo ) 2.37 M 0.0539 M M/s 18 Ar 0.339 M 0.784 M | M/sarrow_forward
- A certain reaction is second order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4] Initial rate of reaction 2.41 M 0.733 M 19.0 M/s 0.501 M 0.733 M Mls 0.873 M 2.02 M Mls dlo Ararrow_forwardConsider the rate data at a certain temperature for the reaction 2NO(g) +2H2(g) →N2(g)+2H2O(g) Experiment [H₂] (M) 1 0.200 2 3 DHONOM 0.200 0.400 Determine the order of the reaction with respect to hydrogen... 1 2 [NO] (M) 0.200 3 0.400 0.400 Rate (M/s) 2.06x10-4 8.24x10-4 1.65×10-3arrow_forwardⒸ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Dataarrow_forward
- 15. What data should be plotted to show that experimental concentration data fits a first-order reaction? A. 1/[reactant] vs. time B. [reactant] vs. time C. ln[reactant] vs. time D. ln(k) vs.1/T E. ln(k) vs. Eaarrow_forward[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.arrow_forwardGood hand written explanation Asap Thanksarrow_forward
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