a. If the current atmospheric pressure was 29.45" of Hg,what is the pressure (torr) of dry hydrogen in the buret? 4. You collect a sample of hydrogen gas in an inverted buret by displacementof water at 29.0 °C. The buret could not be submerged deep enough in thewater bath to equilize pressure. The water level in the buret was 14.76 cmabove the water level in the water bath. The volume of gas in the buret wasdetermined to be 32.60 ml.

Introduction : We have to calculate pressure of dry hydrogen .

4. You collect a sample of hydrogen gas in an inverted buret by displacement of water at 29.00 °C. The buret could not be submerged deep enough in the water bath to equilize pressure. The water level in the buret was 14.76 cm above the water level in the water bath. The volume of gas in the buret was determined to be 32.60 mL.

4. You collect a sample of hydrogen gas in an inverted buret by displacement of water at 29.00 °C. The buret could not be submerged deep enough in the water bath to equilize pressure. The water level in the buret was 14.76 cm above the water level in the water bath. The volume of gas in the buret was determined to be 32.60 mL.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 67QRT

See similar textbooks

Similar questions

93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?
If equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.
You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?