The volume of 1 mole gas at 1atm (atmosphere) and 273.15K (Kelvin) is approximately 22.4 liters. This is known as the molar volume of an ideal gas at standard temperature and pressure (STP).
1atm and 273.15K are commonly used as standard conditions for measuring gas volume because they represent typical atmospheric pressure and room temperature. This allows for easier comparison and calculation of gas volumes in different experiments.
According to the ideal gas law, increasing the temperature or pressure of a gas will result in an increase in volume. Similarly, decreasing the temperature or pressure will result in a decrease in volume. However, this relationship may not hold true for real gases at high pressures or low temperatures.
No, the molar volume of a gas at STP is only applicable to ideal gases. Real gases deviate from ideal behavior at high pressures or low temperatures, so their volumes may differ from the ideal molar volume at STP.
To calculate the volume of a gas at different temperatures and pressures, you can use the ideal gas law: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. This equation can also be rearranged to solve for any of the variables, depending on the given information.