Hello

Im having trouble answering these two questions for my chemistry review. Any help would be greatly appreciated.

(1) Which of the following accounts for the fact that Boyle's Law predicts volumes that are smaller than those observed experimentally at high pressures?

a) Gas molecules are continually colliding with the walls of the container in which they are found.

b) Molecules move at low velocities.

c) There are attractive forces between molecules.

d) Different molecules have different kinetic energies.

e) Molecules have finite volume.

Ive never really understood Boyles Law (even though Ive read up on it many times) so this question stumps me.

The other question below I have no idea how to approach - I suspect it has something to do with limiting reactant but I am confused as to what to do.

2) 47.06 mL of 0.500 M AgNO3 is added to 270.00 mL of water which contains 5.832 g of K2CrO4. A red precipitation of Ag2CrO4 forms. What is the concentration, in mol/L, of unprecipitated CrO4 (charge of -2). Assume Ag2CrO4 is completely insoluble.

Ans.1 If molecules have attractive forces among them, they can not exert as much pressure as they can in absence of those forces. Hence pressure is affected negatively.
If molecules have significant volume,they can not be compressed beyond their volume. Hence Boyle's law does not work for 1c and 1e in your question 1.
Ans.2 you have 0.02353moles of Ag ions in first solution while 0.03 moles of chromate ions in second solution. On mixing the two 0.02353 moles Ag ions need only 0.01176 moles of chromate ions( half of Ag). Now 0.0183 moles of chromate are left in total solution-317.06 mL. To calculate molarity we are to calculate moles in 1000mL of soltion and that is 0.0577moles chromate ions per liter solution.