Why Dalton's law of partial pressure is obeyed by those gases which don't have attractive force?
Answers
Explanation:
Real gases behave ideally when the gases are at low pressure and high temperature. Therefore at high pressures and low temperatures, Dalton's law is not applicable since the gases are more likely to react and change the pressure of the system.
Answer:
Is Dalton's law of partial pressure applicable for only ideal gases? Does the mixture of nitrogen and oxygen obey this law?
Applicable? What do you mean by that word?
Is the ideal gas equation, which is (obviously) concerned with ideal gases, “applicable” only for ideal gases?
There are no ideal gases. Some — large or very polar molecules — are less ideal than others, but none is ideal. There is no such thing as a point mass. There is no such thing as non-interacting molecules.
Yet the ideal gas equation provides a very good approximation of real gas behavior when temperature is moderate to high and pressure is moderate to low.
The same can be said of Dalton’s law of partial pressures. Nitrogen and oxygen are not especially large molecules and are completely nonpolar, so they would be expected to obey ideal gas laws much better than bigger polar molecules.
Explanation: Dalton's law of partial pressure is not applicable at room temperature for a mixture of reacting gases.
Thus, Dalton's law of partial pressure is not applicable at room temperature for a mixture of (A) hydrogen chloride and ammonia.