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Chapter 5: Problem 43

A volume of \(0.280 \mathrm{~L}\) of a gas at STP weighs \(0.400 \mathrm{~g}\). Calculate the molar mass of the gas.

Short Answer

Expert verified
The molar mass of the gas is 32 g/mol.

Step by step solution

01

Calculate the Number of Moles

At standard temperature and pressure (STP), one mole of any gas occupies 22.4 liters. Therefore, we can find out how many moles of gas we have by dividing the given volume by the molar volume: Number of moles = Volume / Molar volume = 0.280 L / 22.4 L/mol = 0.0125 mol.
02

Calculate the Molar Mass

Molar mass is calculated by dividing the mass of the substance by the number of moles. Therefore, molar mass = mass / number of moles = 0.400 g / 0.0125 mol = 32 g/mol.

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Most popular questions from this chapter

State the following gas laws in words and also in the form of an equation: Boyle's law, Charles's law, Avogadro's law. In each case, indicate the conditions under which the law is applicable, and give the units for each quantity in the equation.

Write the ideal gas equation and also state it in words. Give the units for each term in the equation.

Discuss the following phenomena in terms of the gas laws: (a) the pressure in an automobile tire increasing on a hot day, (b) the "popping" of a paper bag, (c) the expansion of a weather balloon as it rises in the air, (d) the loud noise heard when a lightbulb shatters.

A 2.10-L vessel contains \(4.65 \mathrm{~g}\) of a gas at \(1.00 \mathrm{~atm}\) and \(27.0^{\circ} \mathrm{C}\). (a) Calculate the density of the gas in grams per liter. (b) What is the molar mass of the gas?

Why is the density of a gas much lower than that of a liquid or solid under atmospheric conditions? What units are normally used to express the density of gases?
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