the water for 5-8 minutes. Take the temperature of the water at the end of the time boiling. Shut off the gas and allow the water to stop boiling. After boiling has ceased, remove the flask from the beaker. Dry off the flask and let it sit on the bench. Note as the flask cools, the gas should begin to condense into liquid. Once the flask is at room temperature, take the mass. Once the flask has been weighed, place any liquid inside in the respective waste container. To find the volume of the flask, fill it with tap water to the very top. Once it has been filled, empty it into a 250 ml graduated cylinder and record the volume from the cylinder. Make sure to record the barometric pressure written on the board so that you are able to complete your calculations. Now that you have completed the process for the first trial, repeat the process for a second trial. Once you have finished your second trial, return the copper wire and aluminum foil to the stock counter. Waste: All unknown liquid must be placed in the waste container in fume hood 1. Work-up: Determine the number of moles and molar mass of unknown gas for both trials. Determine the average molar mass. Post-Lab Questions: 1. Why does a soda bottle form fizz after you shake it or make a hissing sound (like letting air out of a tire) when you first open it? Hint: explain in terms of gases. wan 2. Have you ever wondered how much pressure a soda bottle can withstand? (depending on the bottle, it is approximately 30 atm. That is 30 times the pressure of the atmosphere on any given day outside!). If you place 15 grams of Zinc solid in a 2.0 L soda bottle with 100 mL of 5 M hydrochloric acid, would the soda bottle be able to withstand the pressure (the gas formed is hydrogen)? The temperature of the collected gas is 25°C. Write and balance the chemical reaction that would take place (you will need this information to help you solve the problem).

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter15: Gases,liquids, And Solids

Section: Chapter Questions

Problem 85E

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Please help me answer these lab questions The Ideal Gas Law experiment

the water for 5-8 minutes. Take the temperature of the water at the end of the time boiling.
Shut off the gas and allow the water to stop boiling. After boiling has ceased, remove the flask
from the beaker. Dry off the flask and let it sit on the bench. Note as the flask cools, the gas
should begin to condense into liquid. Once the flask is at room temperature, take the mass.
Once the flask has been weighed, place any liquid inside in the respective waste container.
To find the volume of the flask, fill it with tap water to the very top. Once it has been filled,
empty it into a 250 mL graduated cylinder and record the volume from the cylinder.
Make sure to record the barometric pressure written on the board so that you are able to
complete your calculations.
Now that you have completed the process for the first trial, repeat the process for a second
trial. Once you have finished your second trial, return the copper wire and aluminum foil to the
stock counter.
Waste:
All unknown liquid must be placed in the waste container in fume hood 1.
Work-up:
Determine the number of moles and molar mass of unknown gas for both trials. Determine
the average molar mass.
Post-Lab Questions:
1. Why does a soda bottle form fizz after you shake it or make a hissing sound (like letting
air out of a tire) when you first open it? Hint: explain in terms of gases.
2. Have you ever wondered how much pressure a soda bottle can withstand? (depending
on the bottle, it is approximately 30 atm. That is 30 times the pressure of the
atmosphere on any given day outside!). If you place 15 grams of Zinc solid in a 2.0 L
soda bottle with 100 mL of 5 M hydrochloric acid, would the soda bottle be able to
withstand the pressure (the gas formed is hydrogen)? The temperature of the collected
gas is 25°C. Write and balance the chemical reaction that would take place (you will
need this information to help you solve the problem).
63

3. How are volume and temperature of an ideal gas related?
4. Is the molar mass you calculated from your data of the unknown gas the same for both
trials? If not, why do you think the values might be different?
5. If the barometric pressure was accidently measured lower than the actual value in lab,
how would the molar mass of the unknown gas be altered?
6. Would the molar mass of the unknown gas be higher or lower if your lab partner
accidently read the temperature as 99.9°C versus the correct value of 99.0°C. Please
explain using the relationships of the ideal gas law and molar mass equation.

Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature

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