What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?

An effective collision between reactant particles requires the particles to have the proper energy and orientation. The particles must have the minimum energy to collide with each other and proper orientation to overlap.

What is collision ?

Collision is a short term force acting between two object when they hit together. According to the kinetic molecular theory of matter, only effective collisions leads to the chemical bonding between atoms.

To make effective collisions, the atoms or constituent particles must acquire a minimum amount of energy  to overcome the barrier potential of reaction.

Similarly, the particles must have proper orientation to have overlapping between their valence shell and form chemical bonds. Inappropriate orientation does not leads to the formation of bond between particles. Hence, option 4 is correct.

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Answer: the fourth stament, The theoretical yield is calculated from the amount of the limiting reactant present.

Justification:

1) Limiting reactant is the one that is in less proportion than the theoretical mole ratio.

2) Excess reactant is the one that is in greater proportion than the theoretical ratio.

3) For example, if you have the equation A + 2B → C, means that 1 mol of A react with 2 moles of B to yield 1 mol of C.

As per that equation, the theoretical mole ratio is 1 mol of A : 2 moles of B : 1 moles of C.

If the actual amounts of A and B were 2 and 4, respectively, they were in the same ratio as the theoretical ratio, and all of the both reactants could react.

But if you had, for example, 2 moles of reactant A and 2 moles of reactant B, only one of the moles of A could react with the 2 moles of B, so B would be the limiting reactant: the whole 2 moles of B would react, while only 1 mole of A would reactant, and 1 mole of A would be left over (A is in excess).

Therefore, you cannot use the 2 moles of A to calculate the theoretical yield (since only 1 mole reacted), instead you must use the limiting reactant (B), which is the one that reacts completely.