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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 = Part A mss volume Calculate the density of oxygen, O2, under each of the following conditions: 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 • STP • 1.00 atm and 20.0 °C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma. • View Available Hint(s) PV = nRT which can be rearranged as ν ΑΣφ ? PV n = RT density at STP, density at 1 atm and 20.0 °C = g/L 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 n is the number of moles and V is the volume, and convert from moles per unit volume to grams per unit volume using molar Part B mass To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 1.90 atm and 22.0 °C and weighed it again. The difference in mass was 9.1 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ?

Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density = Part A mss volume Calculate the density of oxygen, O2, under each of the following conditions: 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 • STP • 1.00 atm and 20.0 °C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma. • View Available Hint(s) PV = nRT which can be rearranged as ν ΑΣφ ? PV n = RT density at STP, density at 1 atm and 20.0 °C = g/L 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 n is the number of moles and V is the volume, and convert from moles per unit volume to grams per unit volume using molar Part B mass To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 1.90 atm and 22.0 °C and weighed it again. The difference in mass was 9.1 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter8: Properties Of Gases
Section: Chapter Questions
Problem 119QRT
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Please answer question 7 Part A and B

Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density Part A mass volume Calculate the density of oxygen, O2, under each of the following conditions: The molar mass of a substance, however, is a STP 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 1.00 atm and 20.0 °C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma. • View Available Hint(s) PV = nRT which can be rearranged as ΑΣφ ? PV п — RT density at STP, density at 1 atm and 20.0 °C = g/L 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 n is the number of moles and V is the volume, and convert from moles per unit volume to grams per unit volume using molar Part B mass To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 1.90 atm and 22.0 °C and weighed it again. The difference in mass was 9.1 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ΑΣφ 画
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 Part A mass volume Calculate the density of oxygen, O2, under each of the following conditions: The molar mass of a substance, however, is a STP 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 1.00 atm and 20.0 °C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma. • View Available Hint(s) PV = nRT which can be rearranged as ΑΣφ ? PV п — RT density at STP, density at 1 atm and 20.0 °C = g/L 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 n is the number of moles and V is the volume, and convert from moles per unit volume to grams per unit volume using molar Part B mass To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 1.90 atm and 22.0 °C and weighed it again. The difference in mass was 9.1 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ΑΣφ 画
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