Answer: Option (a) is the correct answer.
Explanation:
Under conditions of low pressure and high temperature, gas molecules exhibit negligible attractions or repulsions among themselves. Hence, gases behave ideally in these scenarios.
Conversely, at low temperatures, there is a reduction in the kinetic energy of gas molecules, while high pressure compels the molecules to be closer together.
Thus, attractive forces emerge between molecules in conditions of low temperature and high pressure, causing gases to be termed real gases.
Therefore, we conclude that the ideal gas law becomes less accurate when pressure increases and temperature decreases.
Answer:
The temperature of the gas rises.
Explanation:
This is classified as an ISOCHORIC process where the volume remains unchanged. There is no work done by the system.
The gas only receives internal energy from the heat transferred to it from the surroundings.
In this situation, the pressure also increases.
The energy needed to vaporize 1.5 kg of aluminum amounts to 16.345 GJ. The heat of vaporization for aluminum is given as ΔHvap = 294000 kJ/mol. The mass of aluminum in this case equals 1.5 kg which converts to 1500 g. We can calculate the number of moles of aluminum using the formula: Mass of aluminum/(Molar Mass of aluminum). The Molar Mass of aluminum stands at 26.98 g/mol. Using this information, Number of moles calculates to 1500/26.98, which equals 55.6 moles. The total energy required can be expressed as the product of the heat of vaporization and the number of moles of aluminum, so the energy required calculates to 294000 × 55.6, resulting in 16345441.0675 kJ or approximately 16.345 GJ.
