Question

Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 78%. Suppose 10.0 g of A are reacted with excess Compound B, and 12.9g of Compound C are successfully isolated at the end of the reaction.

1. What was the theoretical yield of C?
2. How much B was consumed by the reaction?

Answer 1

Answer:

1. 16.54 grams.

2. 6.64 grams.

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

$A+B\rightarrow C$

Thus, with the given information, the theoretical yield of C is:

$m_C^{theoretical}=\frac{12.9g}{0.78}=16.54g$

Moreover, by considering the law of conservation of mass, the mass at the beginning of the reaction equals the mass at the end of the reaction, therefore, the mass of B that was consumed was:

$m_B=m_C-m_A=16.54g-10.0g=6.64g$

Best regards.

Answer 2

In the given case, 1. the theoretical yield of C = 16.54

2. B was consumed by the reaction = 6.54

A reaction's percent yield essentially tells you many grams of a given product will actually be produced instead of a theoretical  100 g  of product.

• to calculate a reaction's percent yield by dividing the actual yield, which is what the reaction actually produces, by the theoretical yield, which is what the reaction should theoretically produce, and multiplying the result by 100

yield % = $\frac{what\ you\ actually\ get}{what\ you\ should\ theoretically\ get}$  ×100

given:

yield % =78%

actually get C = 12.9 g

should get or theoretical yield = ?

A = 10.0 g

Solution:

1. putting value in formula:

78% = $\frac{12.9}{x}$  ×100

x = $\frac{12.9*100}{78}$

= 16.54

2. Now we have A we have C that are; 10 and 16.54 grams then we can calculate be find the difference between product and reactant A.

=> A + B = C

=> B = 16.54 - 10

=> B = 6.54

Thus, 1. the theoretical yield of C = 16.54

2. How much B was consumed by the reaction = 6.54

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