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...
Related questions
Question
How do I calculate the molarity of the solution
![e of Dioxygen
Name
Name
Separations of Food Dyes by Paper Chromatography
9-1
Date
Sources of Error
There are two sources of error in this experiment, which fortuitously almost cancel one another. Circle the cor-
rect answer in the following statements.
(a) Initially the flask that you weigh is filled with air. At the end of the reaction it is filled with oxygen.
Because oxygen is denser than air, at the end of the reaction the flask is (heavier, lighter) than it would be if
filled with air.
(b) If the oxygen that is evolved is saturated with water vapor, some water will be carried over as well as
evolved oxygen. At the end of the reaction, this effect would cause the flask to be (heavier, lighter) than if
no water were carried over.
Calculate the molarity of a solution that is 3.0 % hydrogen peroxide by weight (3 g H2O2/100 g solution), assum-
ing that the density of the solution is 1.00 g/mL. For one of your trials, calculate the moles of hydrogen per-
oxide that you put in the flask, the moles of oxygen evolved, and the ratio mol O2/mol H2O2. Is the value you
calculate for the ratio consistent with the stoichiometry of the decomposition reaction?
H₂O2(aq) H₂O(1) + O2(g)
eviations from the Ideal Gas Law
real gases deviate to some extent from the behavior of perfect gases. At standard conditions, the density o
g) is 0.0014290 g/mL, that of H2(g) is 0.00008988 g/mL, and that of CO₂(g) is 0.0019769 g/mL.
(a) Using these values and the exact atomic weights, calculate the molar volume of each of these gases, i
milliliters, to five significant figures.
02](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f605619-bbba-4f43-942e-b505f4944796%2F41583c6a-fa36-41a4-bc01-52a70ae81f01%2Fzmduqjq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:e of Dioxygen
Name
Name
Separations of Food Dyes by Paper Chromatography
9-1
Date
Sources of Error
There are two sources of error in this experiment, which fortuitously almost cancel one another. Circle the cor-
rect answer in the following statements.
(a) Initially the flask that you weigh is filled with air. At the end of the reaction it is filled with oxygen.
Because oxygen is denser than air, at the end of the reaction the flask is (heavier, lighter) than it would be if
filled with air.
(b) If the oxygen that is evolved is saturated with water vapor, some water will be carried over as well as
evolved oxygen. At the end of the reaction, this effect would cause the flask to be (heavier, lighter) than if
no water were carried over.
Calculate the molarity of a solution that is 3.0 % hydrogen peroxide by weight (3 g H2O2/100 g solution), assum-
ing that the density of the solution is 1.00 g/mL. For one of your trials, calculate the moles of hydrogen per-
oxide that you put in the flask, the moles of oxygen evolved, and the ratio mol O2/mol H2O2. Is the value you
calculate for the ratio consistent with the stoichiometry of the decomposition reaction?
H₂O2(aq) H₂O(1) + O2(g)
eviations from the Ideal Gas Law
real gases deviate to some extent from the behavior of perfect gases. At standard conditions, the density o
g) is 0.0014290 g/mL, that of H2(g) is 0.00008988 g/mL, and that of CO₂(g) is 0.0019769 g/mL.
(a) Using these values and the exact atomic weights, calculate the molar volume of each of these gases, i
milliliters, to five significant figures.
02
![The Molar Volume of Dioxygen
Name
Data
Date
Locker
. Section
Instructor_
Data
Mass of flask A, contents, stopper, and glass tube before reaction
Mass of flask A, contents, stopper, and glass tube after reaction
Temperature of the gas in flask A
Temperature of the gas in flask D
Volume of oxygen collected
Barometer reading (temperature of barometer
205
°C)
36
Trial 1
20mc
Trial 2
143.40178 140,44118
143.6420 140.07118
24.3 °C 25.0°C °C
22.6
22.1°C
°C
318.9mL 279.37 mL
754.70 torr 5.06torr
Aqueous vapor pressure at temperature of gas (average the two temperatures) 20.38 torr 21.78 torr
Observations
1. Describe the visible changes that take place during the reaction.
There
is
Fizzy
when the iron (ni) Chloride
reacts with
the
hydrogen peroxide. There
is a visual movement of
the water
being pushed out
und into the beaker.
There
TS
a
and then turns
at the middle Erlenpuyer Flu
dark color initially.
a brisht
brown
2. As the reaction proceeds, does flask A get warmer or cooler to the touch? Does the reaction absorb or evolve
heat (energy)?
The flask
set warmer as the reaction progress.
The reaction.
rs
relasy
heat so it is exothermic](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f605619-bbba-4f43-942e-b505f4944796%2F41583c6a-fa36-41a4-bc01-52a70ae81f01%2Fl4pt1ep_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The Molar Volume of Dioxygen
Name
Data
Date
Locker
. Section
Instructor_
Data
Mass of flask A, contents, stopper, and glass tube before reaction
Mass of flask A, contents, stopper, and glass tube after reaction
Temperature of the gas in flask A
Temperature of the gas in flask D
Volume of oxygen collected
Barometer reading (temperature of barometer
205
°C)
36
Trial 1
20mc
Trial 2
143.40178 140,44118
143.6420 140.07118
24.3 °C 25.0°C °C
22.6
22.1°C
°C
318.9mL 279.37 mL
754.70 torr 5.06torr
Aqueous vapor pressure at temperature of gas (average the two temperatures) 20.38 torr 21.78 torr
Observations
1. Describe the visible changes that take place during the reaction.
There
is
Fizzy
when the iron (ni) Chloride
reacts with
the
hydrogen peroxide. There
is a visual movement of
the water
being pushed out
und into the beaker.
There
TS
a
and then turns
at the middle Erlenpuyer Flu
dark color initially.
a brisht
brown
2. As the reaction proceeds, does flask A get warmer or cooler to the touch? Does the reaction absorb or evolve
heat (energy)?
The flask
set warmer as the reaction progress.
The reaction.
rs
relasy
heat so it is exothermic
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