Question

complete the following table.
mass of sample moles of sample molecules in sample total atoms in sample
4.05 g c₆h₆ 0.0518 3.12×10^22
g 0.213 mol h₂o
g 2.18×10²² molecules co₂
submit answer try another version 2 item attempts remaining

Explanation:

Step1: Calculate total atoms for \(C_6H_6\)

Each \(C_6H_6\) molecule has \(6 + 6=12\) atoms.
Total atoms \(=3.12\times 10^{22}\times12 = 3.74\times 10^{23}\)

Step2: Calculate mass and molecules for \(H_2O\)

Molar mass of \(H_2O\) is \(18.015\ g/mol\).
Mass \(=0.213\ mol\times18.015\ g/mol = 3.84\ g\)
Molecules \(=0.213\ mol\times6.022\times 10^{23}\ mol^{-1}=1.28\times 10^{23}\)
Each \(H_2O\) molecule has \(2 + 1 = 3\) atoms.
Total atoms \(=1.28\times 10^{23}\times3=3.84\times 10^{23}\)

Step3: Calculate moles and mass and total atoms for \(CO_2\)

Moles \(=\frac{2.18\times 10^{22}}{6.022\times 10^{23}\ mol^{-1}}=0.0362\ mol\)
Molar mass of \(CO_2\) is \(44.01\ g/mol\).
Mass \(=0.0362\ mol\times44.01\ g/mol = 1.59\ g\)
Each \(CO_2\) molecule has \(1 + 2=3\) atoms.
Total atoms \(=2.18\times 10^{22}\times3 = 6.54\times 10^{22}\)

Answer:

Mass of Sample	Moles of Sample	Molecules In Sample	Total Atoms In Sample
\(3.84\ g\)	\(0.213\ mol\ H_2O\)	\(1.28\times 10^{23}\)	\(3.84\times 10^{23}\)
\(1.59\ g\)	\(0.0362\ mol\)	\(2.18\times 10^{22}\ molecules\ CO_2\)	\(6.54\times 10^{22}\)