Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density = volume • Part A 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 ist Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00 atm and 15.0 °C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a c PV = nRT • View Available Hint(s) which can be rearranged as PV n= 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. density at STP, density at 1 atm and 15.0 °C = g/L Alternatively, you can use the ratio n/V trom 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 mass Submit Part B To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 3.7-L bulb, then fil the gas at 1.60 atm and 30.0 °C and weighed it again. The difference in mass was 6.7 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ΑΣφ ?
Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density = volume • Part A 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 ist Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00 atm and 15.0 °C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a c PV = nRT • View Available Hint(s) which can be rearranged as PV n= 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. density at STP, density at 1 atm and 15.0 °C = g/L Alternatively, you can use the ratio n/V trom 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 mass Submit Part B To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 3.7-L bulb, then fil the gas at 1.60 atm and 30.0 °C and weighed it again. The difference in mass was 6.7 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ΑΣφ ?
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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Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
Question
![**Understanding Gas Density and Molar Mass Calculations**
*Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since:*
\[
\text{density} = \frac{\text{mass}}{\text{volume}}
\]
*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:*
\[
PV = nRT
\]
*which can be rearranged as*
\[
n = \frac{PV}{RT}
\]
*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 \( n \) is the number of moles and \( V \) is the volume, and convert from moles per unit volume to grams per unit volume using molar mass.*
### Part A
**Objective:** Calculate the density of oxygen, \( O_2 \), under each of the following conditions:
- **STP (Standard Temperature and Pressure)**
- **1.00 atm and 15.0 °C**
*Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.*
(An input box is provided for calculation, and a hint section is available.)
### Part B
**Objective:** To identify a diatomic gas (\( X_2 \)), a researcher conducted the following experiment:
- An empty 3.7-L bulb was weighed.
- The bulb was then filled with the gas at 1.60 atm and 30.0 °C and weighed again.
- The difference in mass was 6.7 g.
*Identify the gas by expressing your answer as a chemical formula.*
(An input box is provided for entering the chemical formula, with a hint section available.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbe5243c1-65b6-49ba-aa5b-abca4f72257e%2F86bcf033-f0a3-46c7-a4df-00cc350d03f5%2Fq46qzh3_processed.png&w=3840&q=75)
Transcribed Image Text:**Understanding Gas Density and Molar Mass Calculations**
*Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since:*
\[
\text{density} = \frac{\text{mass}}{\text{volume}}
\]
*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:*
\[
PV = nRT
\]
*which can be rearranged as*
\[
n = \frac{PV}{RT}
\]
*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 \( n \) is the number of moles and \( V \) is the volume, and convert from moles per unit volume to grams per unit volume using molar mass.*
### Part A
**Objective:** Calculate the density of oxygen, \( O_2 \), under each of the following conditions:
- **STP (Standard Temperature and Pressure)**
- **1.00 atm and 15.0 °C**
*Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.*
(An input box is provided for calculation, and a hint section is available.)
### Part B
**Objective:** To identify a diatomic gas (\( X_2 \)), a researcher conducted the following experiment:
- An empty 3.7-L bulb was weighed.
- The bulb was then filled with the gas at 1.60 atm and 30.0 °C and weighed again.
- The difference in mass was 6.7 g.
*Identify the gas by expressing your answer as a chemical formula.*
(An input box is provided for entering the chemical formula, with a hint section available.)
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