Question

What is the mass of a mole of sucrose $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$?

Answer 1

Given,

• Moles of sucrose $=1\mathrm{mol}$

Step 2: To determine the molar mass of sucrose $\mathbf{\left(}{\mathbf{C}}_{\mathbf{12}}{\mathbf{H}}_{\mathbf{22}}{\mathbf{O}}_{\mathbf{11}}\mathbf{\right)}$.

$$\begin{gathered} \text{Molar mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=(12\times \text{Atomic mass of C})+(22\times \mathrm{Atomic}\text{mass of H})+(11\times \mathrm{Atomic}\text{mass of O}) \\ \text{Molar mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=(12\times 12)+(22\times 1)+(11\times 16) \\ \text{Molar mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=(144+22+176)\mathrm{g}{\mathrm{mol}}^{-1} \\ \text{Molar mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=342\mathrm{g}{\mathrm{mol}}^{-1} \end{gathered}$$

Step 2: To determine the mass of ${\mathbf{C}}_{\mathbf{12}}{\mathbf{H}}_{\mathbf{22}}{\mathbf{O}}_{\mathbf{11}}$.

$$\begin{gathered} \text{Mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=\text{Moles of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\times \text{Molar mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11} \\ \text{Mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=1\mathrm{mol}\times 342\mathrm{g}{\mathrm{mol}}^{-1} \\ \text{Mass of}{\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}=342\mathrm{g} \end{gathered}$$

Therefore, the mass of a mole of sucrose is $342\mathrm{g}$.