Question

Name the law behind the dissolution of $C{{O}_{2}}$ gas in soft drinks under high pressure.

Answer 1

Hint: The gas law which contains terms like temperature (T), pressure (P), volume (V) gives a relation between them, which is $PV=$$nRT$. This is also known as the ideal gas law.

Complete step by step solution:
According to the Henry law at constant temperature the amount of gas that dissolves in a given type and volume of a liquid is directly proportional to the partial pressure of the gas in equilibrium with that liquid. The constant of Henry's law is known as the Henry gas constant \[{{K}_{H}}\].
The mathematical form of Henry law is:
\[{{P}_{a}}={{K}_{H}}[c]\]
Where c is the molar concentration of the gas
\[{{P}_{a}}\] is the partial pressure of the gas.
When the carbonated soft drink beverage bottle is sealed with the cap, it is pressurized by the mixture of air and carbon dioxide. Due to this high partial pressure of carbon dioxide the amount of carbon dioxide dissolved in soft drinks is very high and after the removal of the cap excess carbon dioxide escapes and external pressure decreases. This demonstrates Henry's law.

Hence, the one word answer or the law behind the dissolution of $C{{O}_{2}}$ gas in soft drinks under high pressure is Henry's law.

Note: Henry law is applicable only at moderate temperature and high pressure. If the temperature and pressure is high then the Henry law will fail. And also if a gas reacts with liquid then the Henry law is not responsible for the solubility of that gas in the liquid, Henry law fails under such circumstances.