Problem to be solved and to be checked using Boyle's Law equation: In a J-shaped tube filled with mercury, initially, mercury levels in both limbs are the same. The initial volume of the trapped gas in the closed end is 0.50 L. The volume of the gas decreases to 0.30 L after the addition of mercury from the open end of the tube. Take note that the opened end of the tube is subjected to the atmosphere; thus, the initial pressure is equal to atmospheric pressure (1 atm = 780 mmHg). What will be the final pressure after the changes of the volume happened?

Problem to be solved and to be checked using Boyle's Law equation: In a J-shaped tube filled with mercury, initially, mercury levels in both limbs are the same. The initial volume of the trapped gas in the closed end is 0.50 L. The volume of the gas decreases to 0.30 L after the addition of mercury from the open end of the tube. Take note that the opened end of the tube is subjected to the atmosphere; thus, the initial pressure is equal to atmospheric pressure (1 atm = 780 mmHg). What will be the final pressure after the changes of the volume happened?

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Methane is used as a fuel in most homes. It is burned in a boiler which is commonly located on an external wall in the kitchen. Air is drawn into the boiler from the outside through a tube called a flue, which is also used to get rid of the waste gases from the boiler. Why is it essential that the flue is clear of any obstructions and what would be the consequences of a faulty or blocked flue?
According to KMT, at constant pressure and temperature, the frequency and force of molecule wall collisions are constant. So increasing the number of gaseous molecùles will require a proportional increase in the container volume in order to yield a decrease in the number of collisions per unit area to make up for the increased frequency of collisions. What gas law is KMT explaining? Select the correct answer below: Dalton's law O Avogadro's law Boyle's law O Charles's law
If it takes 10.6 hours for 1.00 L of nitrogen, , to effuse through the pores in a balloon, how long would it take for 1.00 L of krypton, , to effuse under the same conditions?
A 1.66 mol sample of CO2 gas is confined in a 40.4 liter container at 23.4 °C. If the temperature of the gas sample is lowered to 0.300 °C holding the volume constant, the force per molecule-wall collision will: Increase )Decrease O Remain the same O Not enough information to answer this question
Discuss briefly the following phenomenon in terms of the gas laws: The pressure increase in an automobile tire on a hot day. The expansion of a weather balloon as it rise in the air
what is the easiest procedure?
2) What is the final pressure (expressed in atm) of a 3.05 L system initially at 724 mm Hg and 298 K, that is compressed to a final volume of 2.51 L at 273 K? A) B)
Solve using the Boyle's Law 1. A sample of argon gas occupies 34.7 mL at 712 torrs and 42oC. What volume will this gas occupy at the same temperature, but at 745 torrs?
Explain how the volume of the bubbles exhausted by a scuba diver as shown change as they rise to the surface, assuming that they remain intact.
Calculate the mass of water vapor present in 25.9 Lof air at 293 K and at 19.45 torr if the relative humidity is 75%. (Use 4 significant figures in your gas constant.) i bo
Consider the lungs, which can be modeled on a very basic level as a 5.0 L container of a mixture of N2 and O2 gases at 298 K. a) Calculate the pressure inside your lungs if filled with 0.15 mol the gas mixture described above, assuming it behaves ideally. b) Is it reasonable to assume that this gas mixture behaves ideally under these conditions? Why or why not?