Molar Mass and Conversion Factors

The video tutorial explains how to calculate the mass of one molecule of diatomic nitrogen (N2). It begins by determining the molar mass of N2, which is the sum of the atomic masses of two nitrogen atoms. The molar mass is then divided by Avogadro's number to find the mass of a single molecule. The tutorial concludes with the final calculation, emphasizing the small mass of a single molecule of N2.

What is the first step in finding the mass of one molecule of N2?

• Calculate the molar mass of N2

• Find the atomic number of nitrogen

• Measure the temperature of N2

• Determine the volume of N2

How do you calculate the molar mass of diatomic nitrogen (N2)?

• Divide the atomic mass of nitrogen by two

• Add the atomic masses of two nitrogen atoms

• Multiply the atomic mass of nitrogen by three

• Subtract the atomic mass of oxygen from nitrogen

What is the molar mass of a single nitrogen atom?

• 14.01 grams per mole

• 28.02 grams per mole

• 7.00 grams per mole

• 16.00 grams per mole

Why do we use a conversion factor in this calculation?

• To measure the temperature change

• To relate moles to Avogadro's number

• To convert grams to liters

• To find the density of N2

What happens to the units of moles during the conversion process?

• They convert to liters

• They double

• They cancel out

• They remain unchanged

What is the final unit of the mass of one molecule of N2?

• Grams

• Moles

• Liters

• Kilograms

What is the calculated mass of one molecule of N2?

• 14.01 grams

• 4.65 x 10^-23 grams

• 28.02 grams

• 6.02 x 10^23 grams

Why is the mass of one molecule of N2 considered very small?

• Because molecules are microscopic

• Because it is a gas at room temperature

• Because it is measured in liters

• Because nitrogen is a light element