Quantitative Aspects of Chemical Change Worksheet

Molar mass of $\text{H} = 1.01 \text{ g/mol}$
Molar mass of $\text{S} = 32.07 \text{ g/mol}$
Molar mass of $\text{O} = 16.00 \text{ g/mol}$

Number of molecules = $n \times N_{A}$
Number of $\text{H}_{2}\text{SO}_{4}$ molecules = $0.0999 \text{ mol} \times 6.022 \times 10^{23} \text{ molecules/mol}$
Number of $\text{H}_{2}\text{SO}_{4}$ molecules = $6.0159 \times 10^{22} \text{ molecules}$

Each $\text{H}_{2}\text{SO}_{4}$ molecule contains 4 oxygen atoms.
Number of oxygen atoms = Number of $\text{H}_{2}\text{SO}_{4}$ molecules $\times 4$
Number of oxygen atoms = $6.0159 \times 10^{22} \times 4$
Number of oxygen atoms = $\boxed{\mathbf{2.41 \times 10^{23} \text{ atoms}}}$

1.3.1 The percentage hydrogen will REMAIN THE SAME.

1.3.2 The law applied is the Law of Definite Proportions (or Law of Constant Composition).

1.4.1 Concentration is defined as the amount of solute (in moles) dissolved per unit volume of solution (in $\text{dm}^{3}$ or liters).

1.4.2

Molar mass of $\text{Na} = 22.99 \text{ g/mol}$
Molar mass of $\text{O} = 16.00 \text{ g/mol}$
Molar mass of $\text{H} = 1.01 \text{ g/mol}$