For each of the trials I-IV in Part I of the experiment, determine which reactant was limiting and determine the theoretical mass of CO2 which could have been produced in each of these trials. From the volumes of CO2 produced in trials I-IV of Part I, and your answer to question 1, find the mass of CO2 actually produced in each of these trials and find a % yield for each trial. Determine the average % yield for your 4 trials.
For each of the trials I-IV in Part I of the experiment, determine which reactant was limiting and determine the theoretical mass of CO2 which could have been produced in each of these trials. From the volumes of CO2 produced in trials I-IV of Part I, and your answer to question 1, find the mass of CO2 actually produced in each of these trials and find a % yield for each trial. Determine the average % yield for your 4 trials.
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter15: Solutions
Section: Chapter Questions
Problem 10CR
Related questions
Question
![Report Questions
These questions are to be answered on notebook paper and included with
this lab handout as your experiment report. Be sure to show complete setups for
all problem solving. Also, use units and follow all rules of significant figures in
your calculations.
To determine the mass of carbon dioxide (CO2) produced in your trials, you will
need a density value for CO2. Gas densities vary somewhat with temperature and
pressure so I will provide you with a formula that you can use to determine this
quantity at your experimental conditions.
Density of CO2 = k (Patm- Pwater) / T
Where: k 0.706 g K/L torr
Patm
Pwater
%3D
the atmospheric press in torr
the vapor pressure of water at your experimental temperature
%3D
T= the temperature of the water in Kelvin
For your convenience, a brief table of water vapor pressures is included here. A
more complete table is found in the appendices at the end of your text.
Temp (°C)
18
Pwater (torr)
15.5
Temp (°C)
24
Pwater (torr)
22.4
19
16.5
25
23.8
20
17.5
26
25.2
21
18.7
27
26.7
22
19.8
28
28.3
23
21.1
29
30.0
Determine the density of CO2 gas at your experimental conditions.
For each of the trials I-IV in Part I of the experiment, determine which reactant
was limiting and determine the theoretical mass of CO2 which could have been
produced in each of these trials.
From the volumes of CO2 produced in trials I-IV of Part I, and your answer to
question 1, find the mass of CO2 actually produced in each of these trials and find a
% yield for each trial.
Determine the average % yield for your 4 trials.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd9db5004-41b4-46a8-9c5d-150bc716e4bd%2F605ec566-a289-4aeb-aa1b-49767d1e4f1d%2F3h8as7g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Report Questions
These questions are to be answered on notebook paper and included with
this lab handout as your experiment report. Be sure to show complete setups for
all problem solving. Also, use units and follow all rules of significant figures in
your calculations.
To determine the mass of carbon dioxide (CO2) produced in your trials, you will
need a density value for CO2. Gas densities vary somewhat with temperature and
pressure so I will provide you with a formula that you can use to determine this
quantity at your experimental conditions.
Density of CO2 = k (Patm- Pwater) / T
Where: k 0.706 g K/L torr
Patm
Pwater
%3D
the atmospheric press in torr
the vapor pressure of water at your experimental temperature
%3D
T= the temperature of the water in Kelvin
For your convenience, a brief table of water vapor pressures is included here. A
more complete table is found in the appendices at the end of your text.
Temp (°C)
18
Pwater (torr)
15.5
Temp (°C)
24
Pwater (torr)
22.4
19
16.5
25
23.8
20
17.5
26
25.2
21
18.7
27
26.7
22
19.8
28
28.3
23
21.1
29
30.0
Determine the density of CO2 gas at your experimental conditions.
For each of the trials I-IV in Part I of the experiment, determine which reactant
was limiting and determine the theoretical mass of CO2 which could have been
produced in each of these trials.
From the volumes of CO2 produced in trials I-IV of Part I, and your answer to
question 1, find the mass of CO2 actually produced in each of these trials and find a
% yield for each trial.
Determine the average % yield for your 4 trials.
![Data Table
Part I: Determination of % Yield
Trial
Mass of NazCO3 used
Volume of
Volume of CO2 produced
6.00 M HC1
74 ml
182ml
1.089
used
I
5.00 mL
1.292 g
II
5.00 mL
1.420 g
225ml
II
5.00 mL
1.668g
310 ml
IV
5.00 mL
24°C
Temperature of water:
729 torr
Atmospheric Pressure:
Part II: Determination of the Formula Weight of an Unknown Metal Carbonate
2.
Unknown #
Volume of
Volume of CO2 produced
Mass of Unknown
Carbonate used
Trial
6.00 M HCI
Used
180ml
188ml
1.00 g
5.00 mL
II
1.00 g
5.00 mL](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd9db5004-41b4-46a8-9c5d-150bc716e4bd%2F605ec566-a289-4aeb-aa1b-49767d1e4f1d%2Fhutf8l_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Data Table
Part I: Determination of % Yield
Trial
Mass of NazCO3 used
Volume of
Volume of CO2 produced
6.00 M HC1
74 ml
182ml
1.089
used
I
5.00 mL
1.292 g
II
5.00 mL
1.420 g
225ml
II
5.00 mL
1.668g
310 ml
IV
5.00 mL
24°C
Temperature of water:
729 torr
Atmospheric Pressure:
Part II: Determination of the Formula Weight of an Unknown Metal Carbonate
2.
Unknown #
Volume of
Volume of CO2 produced
Mass of Unknown
Carbonate used
Trial
6.00 M HCI
Used
180ml
188ml
1.00 g
5.00 mL
II
1.00 g
5.00 mL
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