25. 600 mL of a gas at 345 kPa will occupy a volume of (A) 1200 mL (B) 300 mL (C) 690 mL (D) 255 mL _mL if the pressure is doubled. 26. J.J. Thomson's experiments with discharge tubes demonstrated that: (A) alpha particles are the nuclei of helium atoms (B) the mass of an atom is concentrated in the hucleus (C) cathode rays are streams of negatively charged particles (D) positive particles are attracted to the cathode

25. 600 mL of a gas at 345 kPa will occupy a volume of (A) 1200 mL (B) 300 mL (C) 690 mL (D) 255 mL _mL if the pressure is doubled. 26. J.J. Thomson's experiments with discharge tubes demonstrated that: (A) alpha particles are the nuclei of helium atoms (B) the mass of an atom is concentrated in the hucleus (C) cathode rays are streams of negatively charged particles (D) positive particles are attracted to the cathode

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter9: The Gaseous State

Section: Chapter Questions

Problem 18P

See similar textbooks

Similar questions

If 456 dm3 of krypton at 101 kPa and 21C is compressed into a 30.1-dm3 tank at the same temperature, what is the pressure of krypton in the tank?
1. A student following the procedure described in this module collected the following data: mass Mg, g 0.0243 initial syringe volume, mL 1.0 final syringe volume, mL 26.5 barometric pressure, torr 754 temperature, K 298 (a) calculate the gas law constant (b) What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K? Use the value for R found in part 1.
Refer to the following equation: Mg (s) + 2HNO3(aq) -> Mg(NO3)2 (aq) + H2 (g) A reaction between 0.359 grams of Mg and 21.12mL of a 0.450M HNO3 solution was conducted in a room witht he following conditions: 27.5 degrees Celius, 723mmHg of atospheric pressure. If .15mL of H2 were collected over water (by the water displacement method), calculate the percent yeild of the reaction. (Pressure H2O at 27.5 degrees Celius = 27.82 mmHg)
1. A student following the procedure described in this module collected the following data: mass Mg, g 0.0243 initial syringe volume, mL 1.0 final syringe volume, mL 26.5 barometric pressure, torr 754 temperature, K 298 Determination#1 The value of the gas law constant (R) is 0.0822 L.atm/mol.K Determination #2 he volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K = 248 mL The results of this experiment are greatly affected by the care with which each of the steps is completed (a) Describe the error that would occur if the magnesium were to slide into the HCl in the test tub before the system is sealed off (b) What would be the effect on the results of a rise in the room temperature from 22.0 celcius, when determination #1 was done, to 25.3 celcius, when determination #2 was made? (c) Why must the surface coating of MgO be removed prior to determining the mass of magnesium used in the experiment? (d) What would be the…
Naturally found uranium consists of 99.274%, 238U, 0.720% 235U, and 0.006% 233U (by mass). As we have seen, 235U is the isotope that can undergo a nuclear chain reaction. Most of the 235U used in the first atomic bomb was obtained by gaseous diffusion of uranium hexafluoride, UF6(g). Part A What is the mass of UF6 in a 40.0-L vessel of UF6 at a pressure of 665 torr at 380 K? Part B What is the mass of 235U in the sample described in part A? The atomic mass of uranium-235 is 235.044 u.
A sample of nitrogen occupied 8.0 Liters at 25° C and 98.7 kPa. What would be the volume at 20°C and 102.7 kPa?
Naturally found uranium consists of 99.274% 238U, 0.720% 235U, and 0.006% 233U. As we have seen, 235U is the isotope that can undergo a nuclear chain reaction. Most of the 235U used in the first atomic bomb was obtained by gaseous diffusion of uranium hexafluoride, UF6(g). (a) What is the mass of UF6 in a 30.0-L vessel of UF6 at a pressure of 695 torr at 350 K? (b) What is the mass of 235U in the sample described in part (a)? (c) Now suppose that the UF6 is diffused through a porous barrier and that the change in the ratio of 238U and 235U in the diffused gas can be described by Equation 10.23 (shown in the attached picture). What is the mass of 235U in a sample of the diffused gas analogous to that in part (a)? (d) After one more cycle of gaseous diffusion, what is the percentage of 235UF6 in the sample?
If I react 20.0 grams of hydrogen with 200. grams of oxygen in the formation of water, what volume of water vapor is produced at 500.K and 1.00 atm?
The density of the air in a ballon need to be less than 0.00121 g/ml to fly at 1.0atm. If the composition of air is 70% N2, and 29% O2, and 1% CO2, what is the density of the hot air in the ballon? Will the ballon be able to fly?
Why does the fusion of heavier atoms require higher temperatures than the fusion of hydrogen? a. Because of their greater mass, their gravitational attraction is stronger. b. Because of their greater positive charge, their Coulomb barrier is higher. c. Because of their greater magnetism, the collisions must be more violent. d. Because of their greater friction, overcoming viscosity is more difficult. e. None of these statements is true
In a collision of sufficient force, automobile air bags respondby electrically triggering the explosive decomposition of sodiumazide (NaN₃) to its elements. A 50.0-g sample of sodium azidewas decomposed, and the nitrogen gas generated was collectedover water at 26C. The total pressure was 745.5 mmHg. Howmany liters of dry N₂ were generated?
Give typed explanation 13.4 g of neon gas is placed in a container at 18 °C and 753 mm Hg. What is the volume of the container (in L)?

SEE MORE QUESTIONS

Recommended textbooks for you

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS