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For my lab, we are supposed to make an introduction about key concepts. Does this make sense?
An ideal gas is a hypothetical gas with molecules of a small size that apply no intermolecular forces. In other words, it is a type of gas that, when kept at a constant temperature, would obey the gas laws exactly. Furthermore, an Ideal Gas (perfect gas) is one which obeys Boyle's Law and Charles' Law exactly. However, no known gas is an ideal gas.
An Ideal Gas obeys the Ideal Gas Law, since an ideal gas can be characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them may be deduced from kinetic theory which is also called the Ideal Gas Law, where PV = nRT. In this formula
P = pressure
V = volume
n = number of moles in the gas
T = temperature
R is the dependent on the units of pressure, temperature and volume. R is also equal to 8.3145 J/mol K if Pressure is in kilopascals(kPa), Volume is in litres(L), Temperature is in Kelvin(K). However, Ris equal to 0.0821 L atm K-1 mol-1 if Pressure is in atmospheres(atm), Volume is in litres(L), Temperature is in Kelvin(K).
The ideal gas law can be viewed as occurring from the kinetic pressure of gas molecules colliding with the walls of a container in accordance with Newton's laws. However, there is also a statistical element in the determination of the average kinetic energy of those molecules. The temperature is taken to be proportional to this average kinetic energy; this invokes the idea of kinetic temperature. One mole of an ideal gas at STP occupies 22.4 liters.
STP (Standard Temperature and Pressure) is used widely as a standard reference point for expression of the
properties and processes of ideal gases. The standard temperature is the freezing point of water and the standard pressure is one standard atmosphere. These can be quantified as follows:
Standard temperature: 0°C = 273.15 K
Standard pressure = 1 atmosphere = 760 mmHg = 101.3 kPa
Standard volume of 1 mole of an ideal gas at STP: 22.4 liters
Addtionally, Dalton's law of partial pressures is law stating that the pressure exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture. The pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature.