Log in
Chemistry
2
answers
0
watching
137
views

A balloon is filled with hydrogen gas and produces the followingchemical reaction between iron and sulfuric acid: Fe(s) + H2SO4(aq)--> FeSO4 (aq) + H2(g). If the balloon had a volume of 4800cubic meters and was filled to a pressure of 1 atm at a temperatureof 0 degrees C, a) what mass of iron (in kg) and how many moles ofsulfuric acid were required to fill it? b) If the total mass thatcan be lifted by a balloon is equal to the difference between themass of gas in the balloon and the mass of air displaced by theballoon, how much mass could by lifted by this balloon and how muchmass could the same balloon lift if it was filled with helium atthe same pressure and temperature. c) using the barometric formulaP= P(initial)e^(-mgh/kt) to estimate the height to which theballoon with a payload of 1000kg can rise when filled withhydrogen. (The balloon will rise until its density equals that ofthe surrounding air) Assume the the temperature of the air does notchange with the altitude. Use an average molar mass for the airbased on 80% N2, 20% O2.

Watch
2
answers
0
watching
137
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
Jarrod Robel
Jarrod RobelLv2
28 Sep 2019
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Which of the following statements best explains why a closed balloon filled with helium gas rises in air?
(a) Helium is a monatomic gas, whereas nearly all the molecules that make up air, such as nitrogen and oxygen, are diatomic.
(b) The average speed of helium atoms is greater than the average speed of air molecules, and the greater speed of collisions with the balloon walls propels the balloon upward.
(c) Because the helium atoms are of lower mass than the average air molecule, the helium gas is less dense than air. The mass of the balloon is thus less than the mass of the air displaced by its volume.
(d) Because helium has a lower molar mass than the average air molecule, the helium atoms are in faster motion. This means that the temperature of the helium is greater than the air temperature. Hot gases tend to rise.


Show transcribed image text

I need help writing a decent conclusion. Every time I submit a lab report the professor slams my conclusion saying it needs work. She wants us to state what the results mean and if they are as expected and explain the possible reasons for variation in your results. The lab is below with data/results. Please, please help.

The Ideal Gas Equation: The Determination of Gas Constant, R

Introduction:

The purpose of this experiment is to determine the gas constant R and the percentage of KClO3 in the KClO3 – KCl – MnO2 mixture using the moles of O2, the original weight of the mixture, and the stoichiometry of the reaction. Consider a plot PV vs. nT for a gas sample where P is the pressure of the gas, V is the volume occupied by the gas, n is the number of moles of gas, and T is the temperature of the gas in Kelvin. If the temperatures and pressures fall in normal ranges, the plot will yield a straight line. Thus, PV = nRT where R is the constant of proportionality between the PV product and the nT product. The object of this experiment is to determine P, V, n, and T for a gas sample and determine the gas constant R, using the equation PV = nRT. The gas sample used will be a sample of oxygen gas generated by the MnO2 catalyzed decomposition of KClO3. Following is the equation of the reaction:

For decomposition of the KClO3 in a KClO3 – KCl – MnO2 mixture, the mass of O2can be determined by taking the difference between the mass of the original mixture and the mass of the residue after the decomposition. This mass is then converted to moles of O2 using the molecular weight of oxygen. The volume of the sample will be determined by water displacement in such a way that the pressure of the sample can be determined from the barometric pressure and the vapor pressure of water. The temperature of the sample will be directly measured.

Procedure:

Assemble the equipment for the apparatus shown in figure 1. With the Florence flask filled to the neck with water, the beaker one-third filled with water, and the pinch clamp open, blow into the tube which connects to the test to create a siphon between the flask and the beaker. Reverse the siphon a few times by raising and lowering the beaker. This will fill the tube connecting the flask and the beaker with water and will also remove air bubbles from the system. Adjust the siphon such that the flask is filled to the neck with water, and close the pinch clamp.

Weigh the eight inch test tube. Add approx. 1.5 grams of the KClO3 – KCl – MnO2mixture to the test tube and weigh the test tube containing the mixture. Record each weight to three decimal places. (Also, be sure and record the sample number for the KClO3 – KCl – MnO2.)

Clamp the test tube to the ring stand, and insert the stopper as shown in figure 1. With the pinch clamp open, raise the level of the beaker such that the water level in the beaker is several inches above the water level in the flask. If a significant amount of water runs into the flask, there is an air leak in the system. If you have an air leak, it must be closed before proceeding. Equalize the pressure in the flask with atmospheric pressure by bringing the water level in the beaker to the same height as the water level in the flask. After closing the pinch clamp, empty and dry the beaker. Open the pinch clamp. A small amount of water will run into the beaker: this will not affect your results since later in this experiment, you will again equalize the pressure in the flask with atmospheric pressure. Ask your instructor to check your apparatus before proceeding.

Heat the mixture with a blue flame until the mixture first begins to melt and then solidifies again; and then heat for an additional 2 mins. (Don’t heat more than 7 mins.) Allow the system to cool for 15 mins. Equalize the pressure with atmospheric pressure, as before; then close the pinch clamp and open the system. Quickly measure the temperature of the gas in the flask; also measure the volume of water in the beaker. Record the barometric pressure reading from professor. Weigh the test tube with the residue and record the mass to three decimal places.

Data/Results:

Trial 1

Weight of test tube

41.912 g

Weight of test tube + mixture

43.343 g

Weight of mixture

1.431 g

Weight of test tube + residue

43.211 g

Weight of oxygen

0.132 g

Moles of oxygen

0.00413 mol

Temperature of water (under oxygen)

21.0 0C

Temperature of oxygen

20.5 0C

Barometric pressure

761.5 torr

Vapor pressure of water

18.7 torr

Pressure of oxygen

742.8 torr

Volume of water displaced

0.101 L

Gas constant, R

61.9

Mass of KClO3 in mixture (use balanced equation)

0.338 g

% of KCLO3 in mixture

23.6 %

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in