A gas sample has a volume of 4250 mL at 15^∘ C and 745 mmHg. What is the final temperature, in d

Name: Problem 73, Chapter 8: Chemistry: An Introduction to General, Organic, and Biological Chemistry
Uploaded: 2020-06-08T19:43:07-08:00
Duration: 1 min 19 s
Channel: David Collins
Description: A gas sample has a volume of 4250 mL at 15^∘ C and 745 mmHg. What is the final temperature, in degrees Celsius, after the sample is transferred to a different container with a volume of 2.50 L and a pressure of 1.20 atm when n is constant? (8.5)

step 1 So here we have a combined gas law calculation also. The number of moles of gas are staying cons

Question

A gas sample has a volume of $4250 \mathrm{mL}$ at $15^{\circ} \mathrm{C}$ and 745 mmHg. What is the final temperature, in degrees Celsius, after the sample is transferred to a different container with a volume of $2.50 \mathrm{L}$ and a pressure of 1.20 atm when $n$ is constant? (8.5)

   A gas sample has a volume of $4250 \mathrm{mL}$ at $15^{\circ} \mathrm{C}$ and 745 mmHg. What is the final temperature, in degrees Celsius, after the sample is transferred to a different container with a volume of $2.50 \mathrm{L}$ and a pressure of 1.20 atm when $n$ is constant? (8.5)

Chemistry: An Introduction to General, Organic, and Biological Chemistry

Karen C. Timberlake 12th Edition

Chapter 8, Problem 73

Instant Answer

Solved by Expert David Collins

06/08/2020

Step 1

The volume should be in liters (L), the pressure should be in atmospheres (atm), and the temperature should be in Kelvin (K). Given: Initial volume, V1 = 4250 mL = 4.25 L (since 1L = 1000mL) Initial temperature, T1 = 15°C = 15 + 273.15 = 288.15 K (since Kelvin = Show more…

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A gas sample has a volume of $4250 \mathrm{mL}$ at $15^{\circ} \mathrm{C}$ and 745 mmHg. What is the final temperature, in degrees Celsius, after the sample is transferred to a different container with a volume of $2.50 \mathrm{L}$ and a pressure of 1.20 atm when $n$ is constant? (8.5)

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Key Concepts

Combined Gas Law

The combined gas law is a method to relate the initial and final states of a gas when the number of moles remains constant. It combines Boyle's law, Charles's law, and Gay-Lussac's law into one equation, allowing you to interconvert pressure, volume, and temperature before and after a change in conditions.

Unit Conversion

Accurate problem solving in gas law applications requires converting all measurements to consistent units. This includes converting volume units (such as milliliters to liters) and pressure units (such as mmHg to atm), so that the values are compatible with the gas law equations.

Temperature Conversion

The use of absolute temperature in Kelvin is essential when applying gas laws because the formulas are derived based on absolute temperature scales. Converting temperatures from degrees Celsius to Kelvin (and vice versa if necessary) is a critical step to ensure the correctness of the calculation.

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