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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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Answer:

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The balanced equation of the reaction is:

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The by the stoichiometry 0.02 mol of O3 will be consumed in 8 seconds.

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3 years ago
A 4.0 L container holds a sample of hydrogen gas at 306 K and 150 kPa. If the pressure increases to 300 kPa and the volume remai
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From the question given above, the following data were obtained:

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Initial pressure (P₁) = 150 kPa

Final pressure (P₂) = 300 kPa

Volume = 4 L = constant

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Since the volume is constant, the final (i.e the new) temperature of the gas can be obtained as follow:

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