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Ch.10 - Gases: Their Properties & Behavior
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.10 - Gases: Their Properties & BehaviorProblema 61
Capitolo 10, Problema 61

Which sample contains more molecules, 3.14 L of Ar at 85.0 °C and 1111 mm Hg pressure or 11.07 g of Cl₂?

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Step 1: Use the ideal gas law to calculate the number of moles of Ar. The ideal gas law is given by the equation PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.
Step 2: Convert the given pressure from mm Hg to atm, as the ideal gas constant R is typically used with pressure in atm. Use the conversion factor 1 atm = 760 mm Hg.
Step 3: Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.
Step 4: Rearrange the ideal gas law equation to solve for n (number of moles): n = PV / RT. Substitute the values for P, V, R, and T to find the moles of Ar.
Step 5: Calculate the number of moles of Cl₂ using its molar mass. The molar mass of Cl₂ is approximately 70.90 g/mol. Divide the given mass of Cl₂ by its molar mass to find the moles of Cl₂.

Concetti chiave

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Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law allows us to calculate the number of moles (n) of a gas when we know its pressure (P), volume (V), and temperature (T). Understanding this concept is essential for comparing the number of molecules in different gas samples.
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Ideal Gas Law Formula

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For example, the molar mass of Cl₂ is approximately 70.9 g/mol. Knowing the molar mass allows us to convert between grams of a substance and the number of moles, which is crucial for determining how many molecules are present in a given mass.
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Molar Mass Concept

Avogadro's Number

Avogadro's Number, approximately 6.022 x 10²³, is the number of molecules in one mole of a substance. This constant is fundamental in chemistry for converting between moles and molecules. By using Avogadro's Number, we can easily find the total number of molecules in a sample once we have calculated the number of moles.
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Avogadro's Law
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