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.

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 = 25 g

Molar mass of P = 30.97 g/mole

Molar mass of = 71 g/mole

Molar mass of = 208.24 g/mole

First we have to calculate the moles of and .

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 5 moles of react with 2 moles of

So, 0.352 moles of react with moles of

That means, in the given balanced reaction, 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 .

As, 5 moles of react with 2 moles of

So, 0.352 moles of react with moles of

Now we have to calculate the mass of .

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

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

the current is 0.6

voltage ÷ resistance = current

so 12 ÷ 20 = 0.6