1. A sample of oxygen has a volume of 4.68 L at a pressure of 1520. mm Hg. What would be the pressure of this gas if it were allowed to expand to 10.0 L? (Assume that the temperature remained constant.) 2. A gas is held at a constant temperature while its volume decreases from 450. L to 200. L. What will the final pressure be if the initial pressure is 12.1 atm? 3. A gas at constant temperature occupies a volume of 2.40 L and exerts a pressure of 1.10 atm. What volume will the gas occupy at a pressure of 0.795 atm? 4. If the temperature remains constant, what volume will 42.3 L of a gas at 2.4 atm occupy at standard pressure? 5. A gas with a pressure of 500 torr has a volume of 5.24 L. What volume will it occupy at 760 torr?

1. A sample of oxygen has a volume of 4.68 L at a pressure of 1520. mm Hg. What would be the pressure of this gas if it were allowed to expand to 10.0 L? (Assume that the temperature remained constant.) 2. A gas is held at a constant temperature while its volume decreases from 450. L to 200. L. What will the final pressure be if the initial pressure is 12.1 atm? 3. A gas at constant temperature occupies a volume of 2.40 L and exerts a pressure of 1.10 atm. What volume will the gas occupy at a pressure of 0.795 atm? 4. If the temperature remains constant, what volume will 42.3 L of a gas at 2.4 atm occupy at standard pressure? 5. A gas with a pressure of 500 torr has a volume of 5.24 L. What volume will it occupy at 760 torr?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 114AP

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The following figure shows three 1.00-L bulbs connected by valves. Each bulb contains argon gas with amounts proportional to the number of circles pictorially represented in the chamber. All three bulbs are maintained at the same temperature. Unless stated otherwise, assume that the valves connecting the bulbs are closed and seal the gases in their respective chambers. Assume also that the volume between each bulb is negligible. (a) Which bulb has the highest pressure? (b) If the pressure in bulb A is 0.500 atm, what is the pressure in bulb C? (c) If the pressure in bulb A is 0.500 atm, what is the total pressure? (d) If the pressure in bulb A is 0.500 arm, and the valve between bulbs A and B is opened, redraw the figure shown above to accurately represent the gas atoms in all three bulbs. What is P A+P B+P C? Compare your answer in part (d) to that in part (c). (e) Follow the instructions of part (d) but now open only the valve between bulbs B and C.
À 2.50-L volume of hydrogen measured at —196 C is warmed to 100 C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.
Consider two different containers, each filled with 2 moles of Ne(g). One of the containers is rigid and has constant volume. The other container is flexible (like a balloon) and is capable of changing its volume to keep the extemal pressure and internal pressure equal to each other. If you raise the temperature in both containers, what happens to the pressure and density of the gas inside each container? Assume a constant extemal pressure.
A spherical glass container of unknown volume contains helium gas at 25C and 1.960 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25C, it is found to have a volume of 1.75 cm3. The gas remaining in the first container shows a pressure of 1.710 atm. Calculate the volume of the spherical container.
A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 tor. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)
Most mixtures of hydrogen gas with oxygen gas are explosive. However, a mixture that contains less than 3.0 % O2 is not. If enough O2 is added to a cylinder of H2 at 33.2 atm to bring the total pressure to 3-13 atm, is the mixture explosive?

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