2. Balance the following equation and calculate the volume of hydrogen gasproduced from the reaction of 0.425 g of aluminum when completely reacted withexcess hydrochloric acid. The gas was collected over water at 28 °C and a totalpressure of 745 torr.Al (s) +HCl (aq) >AICI3 (aq) +H2 (g)

The balanced chemical reaction is given below.

Answered: 2. Balance the following equation and…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter1: Gases And The Zeroth Law Of Thermodynamics

Section: Chapter Questions

Problem 1.25E

See similar textbooks

Similar questions

Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.
97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.
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)?
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
The compression ratio in an automobile engine is the ratio of the gas pressure at the end of the compression stroke to the pressure in the beginning. Assume that compression occurs at constant temperature. The total volume of the cylinder in an automobile is 350 cm3, and the displacement the reduction in volume during the compression stroke is 309 cm3. What is the compression ratio in that engine?
95 Some engineering designs call for the use of compressed air for underground work. If water containing iron(II) ions is present, oxygen in the compressed air may react according to the following unbalanced net ionic equation: Fe2++H++O2Fe3++H2O (a) Write the balanced net ionic equation. Remember that the amounts of each substance and the charges must balance. (b) Assume all of the oxygen from 650 L of compressed air at 15°C and 6.5 atm is lost by this reaction. What mass of water would be produced? (The mole fraction of oxygen in air is about 0.21.) (c) What will be the final pressure after the loss of the oxygen?

Recommended textbooks for you

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

2. Balance the following equation and calculate the volume of hydrogen gas produced from the reaction of 0.425 g of aluminum when completely reacted with excess hydrochloric acid. The gas was collected over water at 28 °C and a total pressure of 745 torr. Al (s) + HCl (aq) > AICI3 (aq) + H2 (g)