Volume of CO, Gas Produced (mL) (Last Name A-D) Volume of CO, Gas Produced (mL) (Last Name E-L) Volume of CO, Gas Produced (mL) (Last Name M-Z) Time (min) 1 2.9 3.0 7.1 6.4 6.0 |14.2 13.4 9.0 21.3 14.5 12.0 28.4 18.7 15.0 35.5 24.3 18.0 42.6 26.2 21.0 49.7 8. 29.2 24.0 56.8 34.2 27.0 63.9 10 38.0 30.0 71.0 11 41.3 33.0 78.1 12 43.6 36.0 85.2 39.0 42.0 92.3 99.4 13 47.6 14 51.8 106.5 113.6 120.7 15 57.3 45.0 16 60 48.0 17 63.7 51.0 127.8 54.0 57.0 65.9 18 19 20 Steps: 134.9 142.0 67.2 73.2 60.0 a. Open a blank Excel spreadsheet and type your name and section number in row 2. b. Rename the worksheet Last Name_ Carbon Dioxide, c. Enter the data from Table 1 into an Excel Worksheet starting in row 4, placing the time into Column C and the amount of carbon dioxide produced into Column D. Give the table a title. i. The heads of each column should have the name of the quantity, centered and underlined. ii. The numbers in each column should be centered and formatted for the proper number of significant digits. d. Rearrange the Ideal Gas Law (PV = n RT) to solve for n, the number of moles of CO2 produced. i. The temperature (T) of the reaction was 50°C. ii. The pressure (P) of the reaction was 760 mmHg. iii. Enter the volume in Liters (V) into column E. iv. R is a constant and equals 0.0821 L-atm/mol-K
Volume of CO, Gas Produced (mL) (Last Name A-D) Volume of CO, Gas Produced (mL) (Last Name E-L) Volume of CO, Gas Produced (mL) (Last Name M-Z) Time (min) 1 2.9 3.0 7.1 6.4 6.0 |14.2 13.4 9.0 21.3 14.5 12.0 28.4 18.7 15.0 35.5 24.3 18.0 42.6 26.2 21.0 49.7 8. 29.2 24.0 56.8 34.2 27.0 63.9 10 38.0 30.0 71.0 11 41.3 33.0 78.1 12 43.6 36.0 85.2 39.0 42.0 92.3 99.4 13 47.6 14 51.8 106.5 113.6 120.7 15 57.3 45.0 16 60 48.0 17 63.7 51.0 127.8 54.0 57.0 65.9 18 19 20 Steps: 134.9 142.0 67.2 73.2 60.0 a. Open a blank Excel spreadsheet and type your name and section number in row 2. b. Rename the worksheet Last Name_ Carbon Dioxide, c. Enter the data from Table 1 into an Excel Worksheet starting in row 4, placing the time into Column C and the amount of carbon dioxide produced into Column D. Give the table a title. i. The heads of each column should have the name of the quantity, centered and underlined. ii. The numbers in each column should be centered and formatted for the proper number of significant digits. d. Rearrange the Ideal Gas Law (PV = n RT) to solve for n, the number of moles of CO2 produced. i. The temperature (T) of the reaction was 50°C. ii. The pressure (P) of the reaction was 760 mmHg. iii. Enter the volume in Liters (V) into column E. iv. R is a constant and equals 0.0821 L-atm/mol-K
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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Question
Complete the highlighted section D
Transcribed Image Text:Volume of CO, Gas
Produced (mL)
(Last Name A-D)
Volume of CO, Gas
Produced (mL)
(Last Name E-L)
Volume of CO, Gas
Produced (mL)
(Last Name M-Z)
Time (min)
1
2.9
3.0
7.1
6.4
6.0
|14.2
13.4
9.0
21.3
14.5
12.0
28.4
18.7
15.0
35.5
24.3
18.0
42.6
26.2
21.0
49.7
8.
29.2
24.0
56.8
34.2
27.0
63.9
10
38.0
30.0
71.0
11
41.3
33.0
78.1
12
43.6
36.0
85.2
39.0
42.0
92.3
99.4
13
47.6
14
51.8
106.5
113.6
120.7
15
57.3
45.0
16
60
48.0
17
63.7
51.0
127.8
54.0
57.0
65.9
18
19
20
Steps:
134.9
142.0
67.2
73.2
60.0
a. Open a blank Excel spreadsheet and type your name and section number in row 2.
b. Rename the worksheet Last Name_ Carbon Dioxide,
c. Enter the data from Table 1 into an Excel Worksheet starting in row 4, placing the time into
Column C and the amount of carbon dioxide produced into Column D. Give the table a title.
i. The heads of each column should have the name of the quantity, centered and
underlined.
ii. The numbers in each column should be centered and formatted for the proper number
of significant digits.
d. Rearrange the Ideal Gas Law (PV = n RT) to solve for n, the number of moles of CO2
produced.
i. The temperature (T) of the reaction was 50°C.
ii. The pressure (P) of the reaction was 760 mmHg.
iii. Enter the volume in Liters (V) into column E.
iv. R is a constant and equals 0.0821 L-atm/mol-K
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