Chemical Formulas and Molar Mass

The video tutorial explains how to convert the number of molecules of D nitrogen hexaiodide into grams. It begins with writing the chemical formula, followed by calculating the atomic mass of nitrogen and iodine. The tutorial then uses Avogadro's number to estimate moles and performs dimensional analysis for conversion. Finally, it demonstrates the calculation and rounding to significant figures, resulting in the final answer in grams.

What is the correct chemical formula for dinitrogen hexaiodide?

• NI2

• N6I2

• N2I6

• NI6

How many nitrogen atoms are present in one molecule of dinitrogen hexaiodide?

• 2

• 1

• 3

• 6

What is the atomic mass of iodine used in the calculation?

• 14.07 g/mol

• 126.95 g/mol

• 789.44 g/mol

• 6.02 x 10^23 g/mol

What is the total molar mass of dinitrogen hexaiodide?

• 126.95 g/mol

• 789.44 g/mol

• 140.14 g/mol

• 14.07 g/mol

What is Avogadro's number?

• 126.95

• 14.07

• 789.44

• 6.02 x 10^23

How many molecules are approximately in half a mole?

• 7.89 x 10^23

• 1.5 x 10^23

• 6.02 x 10^23

• 3.01 x 10^23

What is the first step in converting molecules to grams?

• Multiply by molar mass

• Divide by Avogadro's number

• Subtract atomic masses

• Add atomic masses

What is the purpose of using Avogadro's number in the conversion process?

• To find the number of atoms

• To calculate atomic mass

• To convert molecules to moles

• To determine the volume

What is the final rounded mass of dinitrogen hexaiodide in grams?

• 132.5 g

• 430 g

• 789.44 g

• 4.3 g

Why is it important to round the final answer to two significant figures?

• To match the precision of the given data

• To simplify the calculation

• To increase accuracy

• To reduce the number of steps