How does extreme pressure affect the volume occupied by a real gas compared to the predictions of the ideal gas law?

a. the true volume of the gas will be higher than predicted by the ideal gas law because the volume of the actual particles is more significant under high pressure.

b. the true volume of the gas will be higher than predicted by the ideal gas law because the attraction between the particles is weaker under high pressure.

c. the true volume of the gas will be lower than predicted by the ideal gas law because the volume of the actual particles is more significant under high pressure.

d. the true volume of the gas will be lower than predicted by the ideal gas law because the attraction between the particles is weaker under high pressure.

The correct answer is A.

Explanation:

Properties of ideal gases have different volumes under very high pressure. These gases take up additional volume when there is high pressure exerted, and the predicted volume of these gases will end up being smaller than the actual values of the gas volumes. Therefore, the true volume of the gases will be higher than the low ones that were predicted, giving your answer A.

i'm pretty sure it is letter c.) car

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.