NO LINKS A sample of helium gas at a pressure of 2.07 atm fills a flask with a volume of 350. at a temperature of 18.0°C. If the gas is transferred to another flask at a pressure of 1.78 atm with a volume of 275 , what will the new temperature of the gas be?

Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? 1)high pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker 2)high pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant 3) low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker 4)low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant