(II) If 61.5 L of oxygen at 18.0^∘ C and an absolute pressure of 2.45 atm are compressed to 48.8

(II) If 61.5 L of oxygen at 18.0^∘ C and an absolute...

(II) If 61.5 $\mathrm{L}$ of oxygen at $18.0^{\circ} \mathrm{C}$ and an absolute pressure of 2.45 atm are compressed to 48.8 $\mathrm{L}$ and at the same time the temperature is raised to $56.0^{\circ} \mathrm{C},$ what will the new pressure be?

Key Concepts

Ideal Gas Law

The ideal gas law (PV = nRT) is a fundamental equation that relates the pressure, volume, and temperature of an ideal gas to the amount of gas present. It provides a framework for understanding how gases behave under varying conditions, which is crucial for solving problems involving gas compression, expansion, heating, or cooling.

Combined Gas Law

The combined gas law is used when the amount of gas is constant and relates the initial and final conditions using the formula (P?V?/T?) = (P?V?/T?). This law is particularly useful in situations where variables such as pressure, volume, and temperature change simultaneously, allowing one to calculate the new state of the gas.

Temperature Conversion (Celsius to Kelvin)

Converting temperatures from Celsius to Kelvin is essential in gas law calculations because the Kelvin scale is an absolute temperature scale. This conversion ensures that the relationships in the ideal gas and combined gas laws are correctly applied, as these laws require temperatures to be measured in Kelvin.

Absolute Pressure

Absolute pressure refers to the total pressure exerted by a gas, including atmospheric pressure. It is used in calculations involving the ideal gas law because it represents the true pressure of the gas system, ensuring accurate problem-solving when conditions such as pressure are involved.