Combined Gas Law Practice Problem: Find New Volume @wbreslyn

Uploaded September 2024 | Updated September 2026, 2 weeks ago

In this video, we'll tackle a combined gas law practice problem. We're given a gas sample with an initial volume, pressure, and temperature (in Celsius), and we'll calculate its new volume when the pressure and temperature change.

Problem:

A sample of gas has a volume of 15.0 L at a pressure of 1.00 atm and a temperature of 27.2 degrees Celsius. What is the new volume if the pressure is raised to 1580 mmHg and the temperature is raised to 356.2 K?

This is a classic example of how to apply the combined gas law, derived from the ideal gas law, when you're given initial pressure, volume, and temperature, and asked to find the new volume under changed conditions. We'll walk through the solution step-by-step, including the necessary temperature conversion, ensuring you understand the process.

Combined Gas Law Practice Problem: Find New Volume

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$Convert 6.0 L to mL (6 Liters to Milliliters) To convert 6 liters (L) to milliliters (mL), you can use the following steps. Note that the L will cancel out as you perform the conversion, leaving only mL: Conversion Factor: 1 liter (L) = 1000 milliliters (mL) Start with the quantity you want to convert (6 L) and set up a ratio where the original unit (L) is in the denominator and the target unit (mL) is in the numerator, using the conversion factor: Conversion factor: 1000 mL / 1 L Write the quantity you want to convert (6 L) as a fraction over 1: 6 L / 1 Multiply this fraction by the conversion factor: (6 L / 1) * (1000 mL / 1 L) Notice that the units of liters (L) in the numerator and denominator cancel out, leaving only the units of milliliters (mL): (6 * 1000) / (1 * 1) mL = 6000 / 1 mL = 6000 mL So, 6 L is equivalent to 6000 milliliters. The units of liters cancel out during the conversion process, leaving only milliliters as the final unit.$

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