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natka813 [3]
3 years ago
14

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 reac

tion is 40%. Suppose 10.0 g of A are reacted with excess Compound B, and 6.4 g of Compound C are successfully isolated at the end of the reaction.
Chemistry
1 answer:
frez [133]3 years ago
7 0

Given :

Compound A reacts with Compound B to form only one product, Compound C.

The usual percent yield of C in this reaction is 40%.

10.0 g of A are reacted with excess Compound B, and 6.4 g of Compound C

To Find :

The theoretical yield of C.

Solution :

We know, % yield is given by :

\%\ yield = \dfrac{actual\ yield}{theoretical\ yield }\times 100

Putting given values , we get :

40 = \dfrac{6.4}{theoretical\ yield }\times 100\\\\theoretical\ yield=\dfrac{6.4\times 100}{40}\\\\theoretical\ yield=16\ g

Therefore, theoretical yield of C is 16 g.

Hence, this is the required solution.

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How many moles are in 3.01 x 10^23 atoms of zinc?
Lerok [7]

Answer:

<h2>0.5 moles</h2>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

n =  \frac{N}{L} \\

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

n =  \frac{3.01 \times  {10}^{23} }{6.02 \times  {10}^{23} }  =  \frac{3.01}{6.02}  \\  = 0.5

We have the final answer as

<h3>0.5 moles</h3>

Hope this helps you

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2 years ago
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Explanation:

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Are the charges in Li2O balanced yes o No?
motikmotik

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