What is the molar mass A student obtained the following results in a Dumas method experiment:mass of flask =195.316 gmass of flask + condensed vapor = 196.032 g%3Dvolume of flask =237 mL temperature of gas = 92.0 °Catmospheric pressure = 748 mm HgCalculate the molar mass of the sample.theer toanswer

given data ;- mass of flask =195.316 g mass of flask + condensed vapours = 196.032 g mass of…

Answered: A student obtained the following…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter11: Liquids And Solids

Section: Chapter Questions

Problem 11.1QE

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Similar questions

Of helium and oxygen gases, which one do you expect to have a larger deviation from ideality at the same high pressure? Is this the same gas that you would expect to have a larger deviation from ideality at moderate pressure? How about at very low pressure?
he following demonstration takes place in a two-step process: rst, solid calcium carbide (CaC2j)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. Second the acetylene gas produced is then ignited with a match, causing the combustion reaction of acetylene with oxygen gas to produce gaseous carbon dioxide and gaseous water. Write the balanced equations for each reaction that is occurring, including all phases. If a 100.0gsample of calcium carbide (CaC2)is initially reacted with 50.0gof water, which reactant is limiting? Now imagine that the final gases produced are collected in a large bulkier and allowed to cool to room temperature. Using the information from part b ( l00.0gof Cec2reacting with 50.0gof H2O), how many liters of carbon dioxide gas were produced in the balloon at a pressure of 1.00atm and 25C?
Helium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?

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A student obtained the following results in a Dumas method experiment: mass of flask = 195.316 g mass of flask + condensed vapor = 196.032 g %3D volume of flask = 237 mL temperature of gas = 92.0 °C atmospheric pressure = 748 mm Hg Calculate the molar mass of the sample.