Boyle's Law Practice Name Abbreviations atm - atmosphere mm Hg - millimeters of mercury torr - another name for mm Hg P1V1 = P2V2 Example 1: 2.00L of a gas is at 740.0 mmHg pressure. What is its volume at 760 mmHg pressure? Answer: this problem is solved by inserting values into P1V1 = P2V2. (740.0 mmHg) (2.00 L) =(760.0 mmHg) (x) Example #1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure? Answer: this problem is solved by inserting values into P,V1 = P2V2. (740.0 mmHg) (2.00 L) =(760.0 mmHg) (x) Problems: 1. A gas occupies 12.3 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg? 2. If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm? 3. A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure becomes 3.0 atm?

Boyle's Law Practice Name Abbreviations atm - atmosphere mm Hg - millimeters of mercury torr - another name for mm Hg P1V1 = P2V2 Example 1: 2.00L of a gas is at 740.0 mmHg pressure. What is its volume at 760 mmHg pressure? Answer: this problem is solved by inserting values into P1V1 = P2V2. (740.0 mmHg) (2.00 L) =(760.0 mmHg) (x) Example #1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure? Answer: this problem is solved by inserting values into P,V1 = P2V2. (740.0 mmHg) (2.00 L) =(760.0 mmHg) (x) Problems: 1. A gas occupies 12.3 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg? 2. If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm? 3. A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure becomes 3.0 atm?

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...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

Boyle's Law Practice
Name
Abbreviations
atm - atmosphere
mm Hg - millimeters of mercury
torr - another name for mm Hg
P1V1 = P2V2
%3D
Example 1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at 760 mmHg pressure?
Answer: this problem is solved by inserting values into P,V, = P2V2.
(740.0 mmHg) (2.00 L) =(760.0 mmHg) (x)
Example #1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure?
Answer: this problem is solved by inserting values into P,V1 =P2V2.
(740.0 mmHg) (2.00 L) =(760.0 mmHg) (x)
Problems:
1. A gas occupies 12.3 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is
increased to 60.0 mm Hg?
2. If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a
pressure of 2.50 atm?
3. A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure becomes 3.00
atm?
4. A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L?
5. 500.0 mL of a gas is collected at 745.0 mm Hg. What will the volume be at standard pressure?
6. Convert 350.0 mL at 740.0 mm of Hg
its new volume at standard pressure.
7. Convert 338 L at 63.0 atm to its new volume at standard pressure.

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