Calculate each of the following quantities for an ideal gas: (a) the volume of the gas, in liters, if 1.50 mol has a pressure of 126.7 kPa at a temperature of -6 °C, (b) the absolute temperature of the gas at which 3.33 * 10^-3 mol occupies 478 mL at 99.99 kPa, (c) the pressure, in pascals, if 0.00245 mol occupies 413 mL at 138 °C.

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of an ideal gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the absolute temperature in Kelvin. This law allows for the calculation of one variable when the others are known, making it essential for solving problems involving gases.

Absolute temperature is a temperature measurement on the Kelvin scale, which starts at absolute zero (0 K), the point at which molecular motion ceases. To convert Celsius to Kelvin, one adds 273.15 to the Celsius temperature. Understanding absolute temperature is crucial in gas calculations, as the Ideal Gas Law requires temperature to be in Kelvin to ensure accurate results.

In gas calculations, it is important to use consistent units for pressure, volume, and temperature. Pressure can be measured in pascals (Pa) or kilopascals (kPa), volume in liters (L) or milliliters (mL), and temperature in Kelvin (K). Converting between these units is often necessary to apply the Ideal Gas Law correctly, ensuring that all variables are compatible for accurate calculations.