The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temp

Name: Problem 52, Chapter 10: Chemistry: An Atoms-Focused Approach
Uploaded: 2020-07-28T21:32:23-08:00
Duration: 3 min 6 s
Channel: Alexandra Roth
Description: The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature. If the initial volume of the gas is 485 mL, what is the final volume of the gas?

step 1 Boyle's Law relates pressure and volume when the two systems in question are at constant tempera

Question

The pressure on a sample of an ideal gas is increased from $715 \mathrm{mmHg}$ to 3.55 atm at constant temperature. If the initial volume of the gas is $485 \mathrm{mL},$ what is the final volume of the gas?

   The pressure on a sample of an ideal gas is increased from $715 \mathrm{mmHg}$ to 3.55 atm at constant temperature. If the initial volume of the gas is $485 \mathrm{mL},$ what is the final volume of the gas?

Chemistry: An Atoms-Focused Approach

Thomas R. Gilbert,… 2nd Edition

Chapter 10, Problem 52

Instant Answer

Solved by Expert Alexandra Roth

07/28/2020

Step 1

We know that 1 atmosphere is equivalent to 760 millimeters of mercury. So, we can set up a conversion factor as follows: \[P_1 = 715 \, \text{mmHg} \times \frac{1 \, \text{atm}}{760 \, \text{mmHg}} = 0.941 \, \text{atm}\] Show more…

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The pressure on a sample of an ideal gas is increased from $715 \mathrm{mmHg}$ to 3.55 atm at constant temperature. If the initial volume of the gas is $485 \mathrm{mL},$ what is the final volume of the gas?

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Key Concepts

Boyle's Law

Boyle's Law states that for a given amount of an ideal gas at constant temperature, the pressure and volume are inversely proportional. This implies that if the pressure of the gas increases, the volume decreases proportionally, and vice versa, as expressed in the equation P1V1 = P2V2.

Unit Conversion

When solving problems involving gas laws, it is important to have consistent units for all measurements. This may involve converting measurements such as pressure from one unit (e.g., mmHg) to another (e.g., atm) to ensure the calculations follow the gas law equations accurately.

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