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Part A Calculate the density of arxygen, Oy, under each of the following conditions: -1.00 am and 35.0 "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 Hi density at STP, density at 1am and 35.0 "C- Submit | ΑΣΦ A chemical reaction does not occur for this question Submit AZO Part B To identify a diatomic gas (X), a researcher canied out the following experiment She weighed an empty 1.7-L bulb, then filed it with the gas at 1.80 atm and 29:0"C and weighed it again. The difference in mass was 35g. Identify the gas Express your answer as a chemical formula. ide Feedback 22 S

Part A Calculate the density of arxygen, Oy, under each of the following conditions: -1.00 am and 35.0 "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 Hi density at STP, density at 1am and 35.0 "C- Submit | ΑΣΦ A chemical reaction does not occur for this question Submit AZO Part B To identify a diatomic gas (X), a researcher canied out the following experiment She weighed an empty 1.7-L bulb, then filed it with the gas at 1.80 atm and 29:0"C and weighed it again. The difference in mass was 35g. Identify the gas Express your answer as a chemical formula. ide Feedback 22 S

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with question A and B in chemistry

 

Welcome | my.REDLANDScc <Homework 7C - Attempt 1 + Gas Density and Molar Mass which can be rearranged as X 08 I Content Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since mass density = 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 Type here to search https://session.masteringchemistry.com/myct/itemView?assignment ProblemID=191597257&attemptNo=1 MasteringChemistry: Homewor X n = 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 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 6: 20 MasteringChemistry: Homewor X + Part A Calculate the density of oxygen, O₂, under each of the following conditions: • STP . 1.00 atm and 35.0 °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 35.0 °C = Submit Part B ΑΣΦ Provide Feedback IVE ΑΣΦ To identify a diatomic gas (X₂), a researcher carried 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 Hint(s) ? A chemical reaction does not occur for this question. Submit ? g/L < 63 ↓ 0 1 of 8 Review | Constants | Periodic Table Next > 7:05 PM 10/21/2022 x =
Transcribed Image Text:Welcome | my.REDLANDScc <Homework 7C - Attempt 1 + Gas Density and Molar Mass which can be rearranged as X 08 I Content Pressure and temperature affect the amount of space between gas molecules, which affects the volume and, therefore, the density of the gas since mass density = 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 Type here to search https://session.masteringchemistry.com/myct/itemView?assignment ProblemID=191597257&attemptNo=1 MasteringChemistry: Homewor X n = 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 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 6: 20 MasteringChemistry: Homewor X + Part A Calculate the density of oxygen, O₂, under each of the following conditions: • STP . 1.00 atm and 35.0 °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 35.0 °C = Submit Part B ΑΣΦ Provide Feedback IVE ΑΣΦ To identify a diatomic gas (X₂), a researcher carried 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 Hint(s) ? A chemical reaction does not occur for this question. Submit ? g/L < 63 ↓ 0 1 of 8 Review | Constants | Periodic Table Next > 7:05 PM 10/21/2022 x =
Expert Solution
Step 1

We can use the Ideal gas equation to solve the problem i.e. 

PV = nRT

where P = Pressure 

V = Volume

n = no. of moles =  mass(m) / molar mass(MM)

R = gas constant = 0.0821 L.atm.mol-1.K-1

T = Temperature

we can determine no. of moles from here and from no. of moles we can find the mass of the gas and finally the

density.

Density = given mass(m) / Volume (L)

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