Physics, 31.07.2019 20:40 rehel5106

Phosphorous reacts with chlorine gas to produce phosphorous pentachloride. calculate the mass of product produced when 25.0 g of phosphorous reacts with 25.0 grams of chlorine. calculate the mass of product produced if the reaction occurred with a 70.5 percent yield.

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Answer from: cmfuentes0816

Answer : The mass of product produced if the reaction occurred with a 70.5 percent yield will be, 20.67 grams.

Explanation : Given,

Mass of P = 25 g

Mass of Cl_2 = 25 g

Molar mass of P = 30.97 g/mole

Molar mass of Cl_2 = 71 g/mole

Molar mass of PCl_5 = 208.24 g/mole

First we have to calculate the moles of and Cl_2 .

$\text{Moles of }P=\frac{\text{Mass of }P}{\text{Molar mass of }P}=\frac{25g}{30.97g/mole}=0.807moles$

$\text{Moles of }Cl_2=\frac{\text{Mass of }Cl_2}{\text{Molar mass of }Cl_2}=\frac{25g}{71g/mole}=0.352moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$2P+5Cl_2\rightarrow 2PCl_5$

From the balanced reaction we conclude that

As, 5 moles of Cl_2 react with 2 moles of

So, 0.352 moles of Cl_2 react with $\frac{2}{5}\times 0.352=0.1408$ moles of

That means, in the given balanced reaction, Cl_2 is a limiting reagent and it limits the formation of products and is an excess reagent because the given moles are more than the required moles.

Now we have to calculate the moles of PCl_5 .

As, 5 moles of Cl_2 react with 2 moles of PCl_5

So, 0.352 moles of Cl_2 react with $\frac{2}{5}\times 0.352=0.1408$ moles of PCl_5

Now we have to calculate the mass of PCl_5 .

$\text{Mass of }PCl_5=\text{Moles of }PCl_5\times \text{Molar mass of }PCl_5$

$\text{Mass of }PCl_5=(0.1408mole)\times (208.24g/mole)=29.32g$

Now we have to calculate the mass of product produced (actual yield).

$\%\text{ yield of }PCl_5=\frac{\text{Actual yield of }PCl_5}{\text{Theoretical yield of }PCl_5}\times 100$

$70.5=\frac{\text{Actual yield of }PCl_5}{29.32g}\times 100$

$\text{Actual yield of }PCl_5=20.67g$

Therefore, the mass of product produced if the reaction occurred with a 70.5 percent yield will be, 20.67 grams.

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Phosphorous reacts with chlorine gas to produce phosphorous pentachloride. calculate the mass of pro...

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