Question

in a certain chemical reaction compound a combines with compound b to produce compound c (and no other products). measurements were taken of the amounts of a and b present before and after a reaction that produced some c:

compound	initial amount	final amount
b	3.0 g	1.8 g

calculate the theoretical yield of c.
round your answer to the nearest 0.1 g.

suppose the percent yield of c in this reaction was 50. %. calculate the actual amount of c that was isolated at the end of the reaction.
round your answer to the nearest 0.1 g.

Explanation:

Step1: Find mass of A and B reacted

For Compound A: Initial = 8.5 g, Final = 0 g. So mass reacted: \( 8.5 - 0 = 8.5 \) g.
For Compound B: Initial = 3.0 g, Final = 1.8 g. So mass reacted: \( 3.0 - 1.8 = 1.2 \) g.

Step2: Determine limiting reactant and theoretical yield

By law of conservation of mass, mass of C (theoretical yield) = mass of A reacted + mass of B reacted.
So, \( 8.5 + 1.2 = 9.7 \) g.

Step3: Calculate actual yield from percent yield

Percent yield = \( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\% \).
Given percent yield = 50.1%, theoretical yield = 9.7 g.
Actual Yield = \( \frac{50.1}{100} \times 9.7 \approx 4.86 \approx 4.9 \) g (rounded to 0.1 g).

Answer:

Theoretical yield of C: \( \boldsymbol{9.7} \) g
Actual amount of C: \( \boldsymbol{4.9} \) g