Which conditions of P and T are most ideal for a gas?
Low P and High T are most ideal for a gas. This is because ideal gas particles experience no intermolecular forces and these conditions are least…
Under which conditions of temperature and pressure would a 1 liter sample of a real gas?
The ideal gas works properly when the inter-molecular interactions between the gas molecules and volume of gas molecule will be negligible. This is possible when pressure is low and temperature is high. Therefore, the correct option is (3) 500 K and 0.1 atm.
Under which conditions of temperature and pressure is a gas most soluble in water?
1 Answer. A gas is most soluble in water under conditions of high pressure, and low temperature.
Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
Answer:High temperature and low pressure. Explanation: The ideal gas equation presupposes that the molecules of a gas are at infinite distances from each other hence they do not interact at all.
Why do real gases deviate from ideal behavior at low temperatures?
At low temperatures, attractions between gas particles cause the particles to collide less often with the container walls, resulting in a pressure lower than the ideal gas value.
Why are gases not ideal?
At relatively low pressures, gas molecules have practically no attraction for one another because they are (on average) so far apart, and they behave almost like particles of an ideal gas. At higher pressures, however, the force of attraction is also no longer insignificant.
What happens when you increase pressure and temperature?
As the temperature increases, the average kinetic energy increases as does the velocity of the gas particles hitting the walls of the container. The force exerted by the particles per unit of area on the container is the pressure, so as the temperature increases the pressure must also increase.
Why are pressure and temperature directly related?
Gay Lussac’s Law – states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature. If you heat a gas you give the molecules more energy so they move faster. This means more impacts on the walls of the container and an increase in the pressure.
What units are used in the ideal gas law?
Units of P, V and T
| Factor | Variable | Units |
|---|---|---|
| Pressure | P | atm Torr Pa mmHg |
| Volume | V | L m³ |
| Moles | n | mol |
| Temperature | T | K |
Are V and T directly proportional?
Boyle’s law states that pressure (P) and volume (V) are inversely proportional. Charles’ law states that volume (V) and temperature (T) are directly proportional. Gay-Lussac’s law states that pressure (P) and temperature (T) are directly proportional.
How do you derive the ideal gas equation?
PV = nRT
- P is the pressure of the ideal gas.
- V is the volume of the ideal gas.
- n is the amount of ideal gas measured in terms of moles.
- R is the universal gas constant.
- T is the temperature.