Which statement correctly describes the actual yield and the theoretical yield of a reaction?

a.) the actual yield is calculated from the reactant amounts, but the theoretical yield must be measured for each instance of a reaction.

b.)the actual yield is calculated from the amount of the limiting reactant, and the theoretical yield is calculated from the amount of the excess reactant.

c.)the actual yield depends on the reaction conditions, but the theoretical yield varies only with reactant amounts.

d.)the actual yield represents the maximum yield possible, and the theoretical yield assumes perfect reaction conditions.

Answer : Option C) The actual yield depends on the reaction conditions, but the theoretical yield varies only with reactant amounts.

Explanation : The theoretical yield of any reaction depends upon the stoichiometric calculation based on the number of moles of all reactants participating in reaction.

The actual yield is the yield which is obtained after the reaction, in which the amount actually produced of a product is the actual yield of the reaction. When a ratio of actual yield to theoretical yield is taken and is expressed in percent it is called percent yield.

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g