If the pressure in the gas tank of the dipper was set very high, the ideal Gas law breaks
down.
Why is this happening?
a) Argon reacts with the walls of the steel vessel at high pressure
b) The molecules would clump together in the center and invalidate the law
c) A steady measurement could not be made as the gas would leak out too quickly
d) The volume occupied by the molecules themselves is no longer negligible

Answer: d) The volume occupied by the molecules themselves is no longer negligible. This most be the answer because a, b and c don't make any sense at all.

Explanation:

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kumaripoojavt kumaripoojavt · Answer 2 · 2022-07-15T13:14:24+02:00

The volume occupied by the molecules themselves is no longer negligible. Hence, option D is correct.

What is an ideal gas equation?

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

The ideal gas law fails at low temperature and high pressure because the volume occupied by the gas is quite small, so the inter-molecular distance between the molecules decreases.

Hence, the volume occupied by the molecules themselves is no longer negligible.

Learn more about the ideal gas here:

https://brainly.com/question/27691721

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