Question

In: Chemistry

Learning Goal: To use Avogadro's number to convert between microscopic units of atoms and molecules to...

Learning Goal:

To use Avogadro's number to convert between microscopic units of atoms and molecules to the macroscopic world of chemical experiments.

A mole is a unit of matter that represents a known number of particles that is large enough to be weighed on a laboratory balance. One mole of substance contains 6.022×1023 formula units, as shown in the following unit factor:

6.022×1023 formula units1 mol substance

The value 6.022×1023 is called Avogadro's number. The term formula unit is a generic phrase that can mean a molecule, atom, ion, or whatever is represented by the chemical formula. For example, a mole of He contains 6.022×1023helium atoms. A mole of N2 contains 6.022×1023 diatomic N2 molecules but double that number of nitrogen atoms.

Part A

A flask contains 0.240 mol of liquid bromine, Br2. Determine the number of bromine molecules present in the flask.

Express your answer numerically in molecules.

  molecules  

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You may know that a million is 106, a billion is 109, and a trillion is 1012. A trillion trillion would be 1024 which is also known as a septillion.

Part B

Calculate the mass of 1.00×1024 (a septillion) molecules of water given that the molar mass of water is 18.02 g/mol.

Express the answer numerically in grams.

  g  

Part C

The fuel used in many disposable lighters is liquid butane, C4H10. How many carbon atoms are in 4.00 g of butane given that the molar mass of butane is 58.12 g/mol?

Express your answer numerically in atoms.

  carbonatoms  

Solutions

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