Mole — Speclore

Reference data and engineering information about mole for chemistry applications.

Overview

Engineering reference data for Mole in chemistry.

$PV = nRT$

Pressure × Volume = moles × gas constant × temperature.

$M = \frac{n}{V}$

Moles of solute per liter of solution.

$pH = -\log_{10}[H^+]$

Measure of acidity.

1 mole of hydrogen gas (H₂) contains Avogadro's number of molecules:

$\text{Number of molecules} = N_A = 6.022141 \times 10^{23} \text{ molecules}$

Thus, for 1 mol of H₂, there are $6.022141 \times 10^{23}$ molecules.

The number of molecules in 1 kg of ethyl alcohol (molecular weight $M = 46.07 \text{ kg/kmol}$ ) is calculated as:

$n = \frac{m}{M} \times N_A \times 1000$

where $m = 1 \text{ kg}$ , and the factor 1000 converts kmol to mol. Substituting the values:

$n = \left( \frac{1}{46.07} \right) \times 6.022 \times 10^{23} \times 1000 = 1.31 \times 10^{25} \text{ molecules}$

At standard temperature and pressure (STP: 0°C and 1 atm), the molar volume of an ideal gas is:

$V_m = 22.414 \text{ L/mol}$

This property is useful for converting between moles and volume for gases under these conditions.