Understanding the Ideal Gas Law and Mole Calculations

The video tutorial explains how to calculate the number of moles and molecules in a breath of air using the ideal gas law. It starts by analyzing the given data: volume, temperature, and pressure. The tutorial then applies the ideal gas law to find the number of moles, followed by a step-by-step calculation using the ideal gas constant. Finally, it converts the moles to molecules using Avogadro's number, ensuring the correct use of significant figures throughout the process.

What is the initial volume of air inhaled by the athlete?

• 1.50 liters

• 2.50 liters

• 2.00 liters

• 1.85 liters

Which law connects pressure, volume, temperature, and moles?

• Avogadro's Law

• Ideal Gas Law

• Charles's Law

• Boyle's Law

What is the ideal gas constant used in this problem?

• 62.36 L·torr/(mol·K)

• 1.987 cal/(mol·K)

• 0.0821 L·atm/(mol·K)

• 8.314 J/(mol·K)

How is the temperature converted from Celsius to Kelvin?

• Add 273

• Subtract 273

• Multiply by 1.8

• Add 100

What is the pressure of the air in torr?

• 754 torr

• 800 torr

• 700 torr

• 760 torr

What is the calculated number of moles of air in the breath?

• 0.0761 moles

• 0.0812 moles

• 0.0700 moles

• 0.0650 moles

How many significant figures are used in the final mole calculation?

• Five

• Two

• Four

• Three

What is Avogadro's number used for converting moles to molecules?

• 6.022 x 10^25

• 6.022 x 10^23

• 6.022 x 10^22

• 6.022 x 10^24

What is the final number of molecules calculated in the breath?

• 4.58 x 10^23

• 4.58 x 10^22

• 4.58 x 10^21

• 4.58 x 10^24

Why is it important to consider significant figures in calculations?

• To avoid using a calculator

• To simplify the process

• To make calculations easier

• To ensure precision and accuracy