The van der Waals equation for real gases recognizes that
(A) the molecular atrractions between paritcles of a gas decreases the pressure exerted by the gas
(B) the non-zero volumes of gas particles effectively decrease the amount of "empty space" between them
(C) gas particles have non-zero volumes and interact with one another
(D) molar volumes of gases of different types are different
(E) All of the above statements are correct
would the correct answer be (E)?
E is the answer, you are correct
Yes, the correct answer is (E) - All of the above statements are correct. The van der Waals equation incorporates the real behavior of gases by considering the attractive forces between gas particles (option A), the non-zero volumes of gas particles (option B), and the interactions between gas particles (option C). It also recognizes that molar volumes of gases of different types can vary (option D).
Yes, the correct answer is (E) - All of the above statements are correct.
The van der Waals equation for real gases is an improvement of the ideal gas law, which takes into account the interactions between gas particles and their non-zero volumes. Let's break down why each statement is correct:
(A) The molecular attractions between particles of a gas decrease the pressure exerted by the gas: In a real gas, the gas particles attract each other due to intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonding. These attractive forces reduce the force of collisions and, therefore, the pressure exerted by the gas.
(B) The non-zero volumes of gas particles effectively decrease the amount of "empty space" between them: Gas particles have a definite volume, which means they occupy some space. In real gases, the particles do not behave as point masses because they have a non-zero size. This results in a decrease in the available volume for the gas to occupy, reducing the amount of "empty space" between gas particles.
(C) Gas particles have non-zero volumes and interact with one another: As mentioned earlier, the gas particles in a real gas have volumes and interact with each other through intermolecular forces. This interaction can affect properties such as pressure, volume, and temperature.
(D) Molar volumes of gases of different types are different: The molar volume refers to the volume occupied by one mole of a substance at a given temperature and pressure. Real gases have different molar volumes because each gas has its own characteristics, such as the size of its particles and the strength of intermolecular forces.
Therefore, all of the above statements are correct, as they encapsulate the key aspects considered by the van der Waals equation for real gases.
(C) says it best; the others are vague or do not tell the whole story.
(D) is not necessarily true, and whatever differences there between are between gases are very small