Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density= 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= 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 dhide by the volume to find density Alternatively, you can use the ratio n/V from the ideal gas equation where 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, O₂, under each of the following conditions: .STP 1.00 atm and 350 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 35.0 "C-0.142,1.3 Submit * Incorrect; Try Again Part B Previous Answers AE ? AZ -ΧΕΙ ΑΣΦ + + O? To identify a diatomic gas (X₂), a researcher canried out the following experiment: She weighed an empty 1.7-L bulb, then filled it with the gas at 1.80 atm and 29.0 "C and weighed it again. The difference in mass was 3.5 g. Identify the gas. Express your answer as a chemical formula. View Available Hints) noreaction A chemical reaction does not occur for this question Submit Previous Answers * Incorrect; Try Again Provide Feedback e/L Review
Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since density= 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= 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 dhide by the volume to find density Alternatively, you can use the ratio n/V from the ideal gas equation where 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, O₂, under each of the following conditions: .STP 1.00 atm and 350 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 35.0 "C-0.142,1.3 Submit * Incorrect; Try Again Part B Previous Answers AE ? AZ -ΧΕΙ ΑΣΦ + + O? To identify a diatomic gas (X₂), a researcher canried out the following experiment: She weighed an empty 1.7-L bulb, then filled it with the gas at 1.80 atm and 29.0 "C and weighed it again. The difference in mass was 3.5 g. Identify the gas. Express your answer as a chemical formula. View Available Hints) noreaction A chemical reaction does not occur for this question Submit Previous Answers * Incorrect; Try Again Provide Feedback e/L Review
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...
Related questions
Concept explainers
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
I need help with part A and B in chemistry
![**Gas Density and Molar Mass**
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
Calculate the density of oxygen, \(\text{O}_2\), under each of the following conditions:
- STP
- \(1.00 \, \text{atm}\) and \(35.0 \, ^\circ\text{C}\)
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.
**Input:**
- Density at STP, density at 1 atm and \(35 \, ^\circ\text{C}\): \(0.\mathbf{142},1.3 \, \text{g/L}\)
**Feedback:**
- Incorrect; Try Again
---
### Part B
To identify a diatomic gas (\(X_2\)), a researcher carried out the following experiment: She weighed an empty \(1.7\text{L}\) bulb, then filled it with the gas at \(1.80 \, \text{atm}\) and \(29.0 \, ^\circ\text{C}\) and weighed it again. The difference in mass was \(3.5 \, \text{g}\). Identify the gas.
**Feedback:**
- A chemical reaction](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcbc9cffe-f157-4023-ae1e-1819ef0454cd%2Fd169fb2f-5d6e-47ed-a609-c6ba050de164%2Fa3c4htu_processed.png&w=3840&q=75)
Transcribed Image Text:**Gas Density and Molar Mass**
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
Calculate the density of oxygen, \(\text{O}_2\), under each of the following conditions:
- STP
- \(1.00 \, \text{atm}\) and \(35.0 \, ^\circ\text{C}\)
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.
**Input:**
- Density at STP, density at 1 atm and \(35 \, ^\circ\text{C}\): \(0.\mathbf{142},1.3 \, \text{g/L}\)
**Feedback:**
- Incorrect; Try Again
---
### Part B
To identify a diatomic gas (\(X_2\)), a researcher carried out the following experiment: She weighed an empty \(1.7\text{L}\) bulb, then filled it with the gas at \(1.80 \, \text{atm}\) and \(29.0 \, ^\circ\text{C}\) and weighed it again. The difference in mass was \(3.5 \, \text{g}\). Identify the gas.
**Feedback:**
- A chemical reaction
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 5 steps with 5 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY