A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 640. mL at a pressure of 1.00 atm, and it weighs 0.712 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 640. mL at a pressure of 1.00 atm, and it weighs 0.712 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

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...

See similar textbooks

Related questions

Q: Sulfur tetrafluoride gas is collected at 25.0 °C in an evacuated flask with a measured volume of…

Q: Some N₂ gas is mixed with some O, gas, and the sketch below shows a representative sample of the…

Q: A 10.0 L tank at 12.5 °C is filled with 3.91 g of sulfur tetrafluoride gas and 6.79 g of dinitrogen…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 3.91 g Mass of dinitrogen monoxide i.e N2O = 6.79 g…

Q: Chlorine pentafluoride gas is collected at −20.0°C in an evacuated flask with a measured volume of…

A: This can be calculated from ideal gas equation : PV = nRT

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point…

Q: A sample of an unknown compound is vaporized at 200. °C. The gas produced has a volume of 1650. mL…

A: The equation of state of a hypothetical ideal gas is known as the ideal gas law. Although it has…

Q: A sample of an unknown compound is vaporized at 160. °C. The gas produced has a volume of 750. mL at…

A: We have to calculate the molar mass of gas.

Q: You are trying to determine, by experiment, the formula of a gaseous hydrofluorocarbon compound you…

A: The objective of the question is to calculateThe molar mass of the compoundThe molecular formula

Q: A sample of argon gas at 55.19 °C has a pressure of 92.56 kPa and occupies 5.71 L. How many moles of…

A: In this question, we want to determine the number of moles of Argon gas You can see details…

Q: Dinitrogen difluoride gas is collected at 13.0 °C in an evacuated flask with a measured volume of…

A: Given Temperature ( T ) = 13 ℃ = ( 13 + 273 ) K…

Q: Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the…

Q: For many purposes we can treat nitrogen N2 as an ideal gas at temperatures above its boiling…

A: Answer:When number of moles of a gas is constant then equation of state for a gas sample is:Here:

Q: Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. R

A: Given: Volume= 30.0 L Pressure= 0.320 atm Temperature= 8.0oC= 281.15 K To calculate:

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point…

A: Data

Q: A sample of an unknown compound is vaporized at 130. °C. The gas produced has a volume of 2080. mL…

A: Given - - > V = 2080 ml = 2.08 L P = 1 atm R = 0.082 L.atm/mol.K T = 130°C = 403.15K molar mass…

Q: A sample of an unknown compound is vaporized at 150. °C. The gas produced has a volume of 1240. mL…

A: Given that : The volume of the gas = 1240 mL The pressure of the gas = 1.00 atm The mass of the gas…

Q: A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 g of dinitrogen…

Q: Sulfur tetrafluoride gas is collected at 23.0 °C in an evacuated flask with a measured volume of…

A: Given that :The temperature of sulfur tetrafluoride gas = 23The volume of the gas = 15.0 LPressure =…

Q: For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point…

A: The relationship between a fixed amount of gas's pressure, volume, and absolute temperature is…

Q: For many purposes we can treat propane (C3H8) as an ideal gas at temperatures above its boiling…

A: Since the given range of temperature is above the boiling point of propane so we can assume it as an…

Q: Four gases, A, B, C and D, are mixed into a sealed container. The total pressure is 3.31. What is…

A: Total pressure of a mixture is the sum of partial pressure of its constituents.

Q: Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: Answer:Dalton's law of partial pressure states that partial pressure of any gas in the gaseous…

Q: A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 2100. mL…

A: The volume of the gas is = 2100 mL The pressure of the gas is = 1.00 atm The mass of the gas is =…

Q: A reaction between liquid reactants takes place at 18.0 °C in a sealed, evacuated vessel with a…

A: Given: Mass of dinitrogen monoxide gas = 10 g Volume of vessel = 45 L Temperature = 18 °C = 18 +273…

Q: Some N₂ gas is mixed with some O2 gas, and the sketch below shows a representative sample of the…

A: given problem solved as Mole fraction = mole of one component ÷ mol of both componentsN 2 = 17÷ (…

Q: A mixture of CH4 (g) and C₂H6 (g) has a total pressure of 0.54 atm. Just enough O2 (g) is added to…

A: Solutions Hence the mole fraction of methane 0.6018

Q: A sample of 0.225 mole of gas has a volume of 748 mL at 28°C. Calculate the pressure in atm of this…

Q: For many purposes we can treat propane (C3H8) as an ideal gas at temperatures above its boiling…

A: Given: The initial pressure = 4.2 atm The initial temperature = -22.0 oC The final temperature =…

Q: calculate the molar mass of the compound.

A: Ideal Gas Law :- PV = nRT P is the pressure of gas V is the volume occupied by gas n is the…

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point…

Q: A sample of an unknown compound is vaporized at 160. °C. The gas produced has a volume of 1200. mL…

A: Given: Volume of ideal gas produced: 1200 ml = 1.2 L Pressure of gas: 1 atm Temperature: 160°C =…

Q: A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 1840. mL…

A: Answer:Here:

Q: An empty glass flask has a mass of 56.52 g and a volume of 875.0 mL. When the flask is filled with…

A: Ideal gases are hypothetical gases which do have real existence. A gas can behave ideally at low…

Q: A 8.00 L tank at 3.9 °C is filled with 17.0 g of sulfur tetrafluoride gas and 7.06 g of boron…

A: Given, Volume of tank = 8.00 L At temperature = 3.9 °C The mass of sulfur tetrafluoride = 17.0 g…

Q: Dinitrogen difluoride gas is collected at 10.0 °C in an evacuated flask with a measured volume of…

Q: Chlorine pentafluoride gas is collected at 26.0 °C in an evacuated flask with a measured volume of…

Q: ome N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the…

Q: A reaction between liquid reactants takes place at 32.0 °C in a sealed, evacuated vessel with a…

Q: A sample of an unknown compound is vaporized at 160. °C. The gas produced has a volume of 1010. mL…

A: Temperature = 160°C Volume = 1010 ml Pressure = 1.00 atm Mass of the unknown compound = 1.43 g…

Q: Chlorine pentafluoride gas is collected at -17.0 °C in an evacuated flask with a measured volume of…

Q: 1. (a) Show the balanced equation for the solubility equilibrium that would occur when a solution of…

A: Applying basics of chemical reaction and determination of Ksp.

Q: A sample of an unknown compound is vaporized at 150. °C. The gas produced has a volume of 1830. mL…

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling…

A: Initial Volume = V1 Final Volume = V2 Initial Temperature = T1 = −14.0°C = (−14.0 + 273.15) K =…

Q: Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the…

A: Mole fraction = mole of species / total moles Partial pressure of specie= mole fraction × total…

Q: 92 and the numerical value of b is 0.0429 . Use the van der Waals equation to calculate…

Q: Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: The mole fractions are calculated using the following formulae.

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 640. mL at a pressure of 1.00 atm, and it weighs 0.712 g.
Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.
x10
mol
Submit Ass
Continue
2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center A-
IMG-4471.jpg
IMG-4467.jpg
IMG-4464.jpg
IMG-4474.jpg
IMG-4472.jpg
MacBook Air
DII
DD
80
F11
F7
F8
F9
F10
F4
F5
F6
F1
F2
F3
%
&
%24

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

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.

Similar questions

For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of −196. °C. Suppose the temperature of a sample of nitrogen gas is raised from -23.0 °C to 22.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.19 kPa and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. kPa x10 × Ś
1. Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00 atmatm and 10.0 ∘C 2. To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 3.8-L bulb, then filled it with the gas at 1.70 atm and 20.0 ∘C and weighed it again. The difference in mass was 7.5 g . Identify the gas. Express your answer as a chemical formula.
A reaction between liquid reactants takes place at 29.0 °C in a sealed, evacuated vessel with a measured volume of 5.0 L. Measurements show that the reaction produced 49. g of sulfur hexafluoride gas. Calculate the pressure of sulfur hexafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits. pressure: atm ?
A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: х10 sulfur tetrafluoride partial pressure: | atm ? mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm
For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is raised from −12.0°C to 21.0°C, and at the same time the pressure is changed. If the initial pressure was 2.5atmand the volume decreased by 45.0%, what is the final pressure? Round your answer to the correct number of significant digits. atm
Boron trifluoride gas is collected at 6.0 °C in an evacuated flask with a measured volume of 15.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.140 atm . Calculate the mass and number of moles of boron trifluoride gas that were collected. Be sure your answer has the correct number of significant digits. mass: g x10 mole: | mol ?
For many purposes, we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C Suppose the pressure on a 440.mL sample of ammonia gas at −8.00°C is tripled. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.
Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 3.00 atm. key carbon hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure x10 N₂ 02 atm ☐ ☑ atm
Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1100. torr. key carbon hydrogen dlo nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr O2 torr
Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 800. torr. gas N₂ 0₂ carbon nitrogen oxygen 0 Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. mole fraction partial pressure torr key torr hydrogen x sulfur chlorine X S OL A
A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 2130. mL at a pressure of 1.00 atm, and it weighs 6.27 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. g x10 mol
A sample of an unknown compound is vaporized at 150. °C. The gas produced has a volume of 2330. mL at a pressure of 1.00 atm, and it weighs 6.37 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. g mol x10 ×