Substances have internal energy due to the constant, random motion of their particles. This is a kind of kinetic energy that differs depending on the substance's state of matter. Arrange the states of matter in order of increasing kinetic energy. liquid gas

Solid < Liquid < gas

Explanation:

Matter consists of molecules, atoms and ions which are held together by forces of cohesion.

The states of matter are solid, liquid and gas.

Solids have molecules, atoms and ions that are tightly packed hence cannot move freely within the structure of the solid particle. This results in low kinetic energy

Liquids have molecules, atoms and ions that are freely packed together compared to solids hence are able to move freely within the structure of the liquid substance to a some extent. This results in a higher kinetic energy compared to that of the solid particle.

Gases have molecules, atoms and ions that are very loosely packed compared to the liquid substance and can move freely within the body of its container. This results in very kinetic energy and increased random motion

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in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm