According to kinetic-molecular theory, which of the following would not be considered an ideal gas? check all that apply. a gas at very high temperatures, when gas particles are moving very quickly a gas at very low volumes, when gas particles are very close together a gas at very low temperatures, when gas particles have very little kinetic energy a gas at very low pressures, when gas particles are very far apart a gas with highly polar molecules that have very strong intermolecular forces

A gas at very low volumes, when gas particles are very close together

A gas at very low temperatures, when gas particles have very little kinetic energy

A gas with highly polar molecules that have very strong inter-molecular forces

Explanation:

According to kinetic molecular theory:

a) Ideal gases have large number of particles which were considered to be hard spherical objects.

b) these gas particles move randomly in a straight line.

c) the path of gas particles change when they collide with each other or walls of vessel.

d) there is no or negligible inter molecular interactions between the gas particles.

e) the inter molecular distances is much higher than the size of particles.

f) the gas particles occupy negligible volume of the vessel.

g) during collision of gas particles is perfectly elastic.

h) the average kinetic energy of particles is constant at a constant temperature. It varies directly with the temperature.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

b.

the accuracy of the data.