Final Exam Review Flashcard - Day 3

Front

What is the atomic mass of Argon (Ar)?

Back

39.948 g

Front

How many molecules are there in 31.8 moles of water?

Back

1.91 x 10^25 molecules

Front

What is the molar mass of CaBr2?

Back

200 g/mole

Front

What is the atomic mass of chromium (Cr)?

Back

51.99 g

Front

To convert from particles to moles, you should multiply by ....

Back

Avogadro's number (6.022 x 10^23) to convert particles to moles.

Front

What is Avogadro's number?

Back

6.022 x 10^23, the number of particles in one mole of a substance.

Front

Define molar mass.

Back

The mass of one mole of a substance, typically expressed in grams per mole (g/mole).

Front

What is the formula to calculate the number of moles?

Back

Number of moles = mass (g) / molar mass (g/mole).

Front

What is the significance of the atomic mass unit (amu)?

Back

It is a standard unit of mass that quantifies mass on an atomic or molecular scale.

Front

How do you calculate the molar mass of a compound?

Back

Add the atomic masses of all atoms in the compound's formula.