Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density = mass volume The molar mass of a substance, however, is a constant and can be used to identify an unknown gas sample. Molar mass is found by dividing the mass of a sample (in grams) by the number of moles in that sample. The number of moles of gas can be calculated using the ideal gas law which can be rearranged as PV = nRT PV n = PT RT Given the number of moles of a gas and its molar mass, you can calculate the mass of the gas. Since density is equal to the ratio of the mass and volume, you can then divide by the volume to find density. Alternatively, you can use the ratio n/V from the ideal gas equation where it is the number of moles and V is the volume, and convert from moles per unit volume to grams per unit volume using molar mass ▼ Part A Calculate the density of oxygen, Oy, under each of the following conditions: . STP . 1.00 atm and 15.0 °C Express your answers numerically in grams per liter to three significant figures. Enter the density at STP first and separate your answers by a comma. View Available Hint(s) density at STP, density at 1 atm and 15.0 °C- Submit Part B ΑΣΦ → A Submit 1957 ΑΣΦ A C Xxx ? To identify a diatomic gas (X₂), a researcher carried out the following experiment: She weighed an empty 4.2-L bulb, then filled it with the gas at 2.00 atm and 27.0 "C and weighed it again. The difference in mass was 9.5 g. Identify the gas. Express your answer as a chemical formula. ▸ View Available Hint(s) www. ? A chemical reaction does not occur for this question. Review | Constants | Periodic Table R/L
Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density = mass volume The molar mass of a substance, however, is a constant and can be used to identify an unknown gas sample. Molar mass is found by dividing the mass of a sample (in grams) by the number of moles in that sample. The number of moles of gas can be calculated using the ideal gas law which can be rearranged as PV = nRT PV n = PT RT Given the number of moles of a gas and its molar mass, you can calculate the mass of the gas. Since density is equal to the ratio of the mass and volume, you can then divide by the volume to find density. Alternatively, you can use the ratio n/V from the ideal gas equation where it is the number of moles and V is the volume, and convert from moles per unit volume to grams per unit volume using molar mass ▼ Part A Calculate the density of oxygen, Oy, under each of the following conditions: . STP . 1.00 atm and 15.0 °C Express your answers numerically in grams per liter to three significant figures. Enter the density at STP first and separate your answers by a comma. View Available Hint(s) density at STP, density at 1 atm and 15.0 °C- Submit Part B ΑΣΦ → A Submit 1957 ΑΣΦ A C Xxx ? To identify a diatomic gas (X₂), a researcher carried out the following experiment: She weighed an empty 4.2-L bulb, then filled it with the gas at 2.00 atm and 27.0 "C and weighed it again. The difference in mass was 9.5 g. Identify the gas. Express your answer as a chemical formula. ▸ View Available Hint(s) www. ? A chemical reaction does not occur for this question. Review | Constants | Periodic Table R/L
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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![Pressure and temperature affect the amount of space between gas
molecules, which affects the volume and, therefore, the density of the
gas since
density = mass
volume
The molar mass of a substance, however, is a constant and can be
used to identify an unknown gas sample. Molar mass is found by
dividing the mass of a sample (in grams) by the number of moles in that
sample. The number of moles of gas can be calculated using the ideal
gas law
which can be rearranged as
PV = nRT
PV
n = PT
RT
Given the number of moles of a gas and its molar mass, you can
calculate the mass of the gas. Since density is equal to the ratio of the
mass and volume, you can then divide by the volume to find density.
Alternatively, you can use the ratio n/V from the ideal gas equation
where it is the number of moles and V is the volume, and convert from
moles per unit volume to grams per unit volume using molar mass
▼
Part A
Calculate the density of oxygen, Oy, under each of the following conditions:
. STP
. 1.00 atm and 15.0 °C.
Express your answers numerically in grams per liter to three significant figures. Enter the density at STP first and separate your answers by a comma.
View Available Hint(s)
density at STP, density at 1 atm and 15.0 °C-
Submit
Part B
ΑΣΦ → A
Submit
[37] ΑΣΦ] A A C
www. ?
To identily a diatomic gas (X₂), a researcher carried out the following experiment: She weighed an empty 4.2-L bulb, then filled it with the gas at 2.00 atm and 27.0 "C
and weighed it again. The difference in mass was 9.5 g. Identify the gas.
Express your answer as a chemical formula.
▸ View Available Hint(s)
A chemical reaction does not occur for this question.
?
Review | Constants | Periodic Table
R/L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F47b0c065-d829-4cdd-bbb4-fc0ba1d88dca%2Fa666e372-0fc7-43cd-9def-23a84e325b3f%2Frv5ldh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Pressure and temperature affect the amount of space between gas
molecules, which affects the volume and, therefore, the density of the
gas since
density = mass
volume
The molar mass of a substance, however, is a constant and can be
used to identify an unknown gas sample. Molar mass is found by
dividing the mass of a sample (in grams) by the number of moles in that
sample. The number of moles of gas can be calculated using the ideal
gas law
which can be rearranged as
PV = nRT
PV
n = PT
RT
Given the number of moles of a gas and its molar mass, you can
calculate the mass of the gas. Since density is equal to the ratio of the
mass and volume, you can then divide by the volume to find density.
Alternatively, you can use the ratio n/V from the ideal gas equation
where it is the number of moles and V is the volume, and convert from
moles per unit volume to grams per unit volume using molar mass
▼
Part A
Calculate the density of oxygen, Oy, under each of the following conditions:
. STP
. 1.00 atm and 15.0 °C.
Express your answers numerically in grams per liter to three significant figures. Enter the density at STP first and separate your answers by a comma.
View Available Hint(s)
density at STP, density at 1 atm and 15.0 °C-
Submit
Part B
ΑΣΦ → A
Submit
[37] ΑΣΦ] A A C
www. ?
To identily a diatomic gas (X₂), a researcher carried out the following experiment: She weighed an empty 4.2-L bulb, then filled it with the gas at 2.00 atm and 27.0 "C
and weighed it again. The difference in mass was 9.5 g. Identify the gas.
Express your answer as a chemical formula.
▸ View Available Hint(s)
A chemical reaction does not occur for this question.
?
Review | Constants | Periodic Table
R/L
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