A 248 -mL gas sample has a mass of 0.433 g at a pressure of 745 mm Hg and a temperature of 28^∘

Name: Problem 57, Chapter 5: Chemistry A Molecular Approach
Uploaded: 2021-10-25T20:31:26-08:00
Duration: 1 min 20 s
Channel: David Collins
Description: A 248 -mL gas sample has a mass of 0.433 g at a pressure of 745 mm Hg and a temperature of 28^∘ C . What is the molar mass of the gas?

step 1 To calculate the molar mass from the density or information that allows us to calculate density,

Question

A 248 -mL gas sample has a mass of 0.433 g at a pressure of 745 $\mathrm{mm} \mathrm{Hg}$ and a temperature of $28^{\circ} \mathrm{C} .$ What is the molar mass of the gas?

   A 248 -mL gas sample has a mass of 0.433 g at a pressure of 745 $\mathrm{mm} \mathrm{Hg}$ and a temperature of $28^{\circ} \mathrm{C} .$ What is the molar mass of the gas?

Chemistry A Molecular Approach

Nivaldo J. Tro 4th Edition

Chapter 5, Problem 57

Instant Answer

Solved by Expert David Collins

10/25/2021

Step 1

The density can be calculated by taking the mass of the gas and dividing it by the volume in liters. Given that the mass of the gas is 0.433 g and the volume is 248 mL (which is equal to 0.248 L), the density is given by: \[ \text{Density} = Show more…

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A 248 -mL gas sample has a mass of 0.433 g at a pressure of 745 $\mathrm{mm} \mathrm{Hg}$ and a temperature of $28^{\circ} \mathrm{C} .$ What is the molar mass of the gas?

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Key Concepts

Ideal Gas Law

The ideal gas law, represented by the equation PV = nRT, is a fundamental relation in chemistry used to describe the behavior of an ideal gas. It connects pressure (P), volume (V), the number of moles (n), and temperature (T) through the gas constant (R), allowing one to calculate any one of these properties when the others are known.

Molar Mass

Molar mass is the mass of one mole of a substance and is calculated by dividing the mass of a sample by the number of moles present. It is a crucial concept for identifying a gas or comparing its experimental properties with theoretical predictions.

Unit Conversions

Unit conversions are essential in gas law problems because pressure, volume, and temperature are often given in different units than those used in the ideal gas constant. Converting quantities to consistent units (e.g., temperature to Kelvin, volume to liters, pressure to atmospheres) ensures the accuracy and consistency of the calculations.

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