Enter your answer in the provided box. roasting galena [lead(ii) sulfide] is an early step in the industrial isolation of lead. how many liters of sulfur dioxide, measured at stp, are produced by the reaction of 5.05 kg of galena with 123 l of oxygen gas at 220°c and 2.00 atm

Answer : The volume of produced are 90.7 liters.

Explanation :

The balanced chemical reaction will be:

First we have to calculate the moles of PbS.

Molar mass of PbS = 239.26 g/mole

Now we have to calculate the moles of by using ideal gas equation.

Using ideal gas equation :

where,

P = Pressure of gas = 2.00 atm

V = Volume of gas = 123 L

n = number of moles   = ?

R = Gas constant =

T = Temperature of gas =

Putting values in above equation, we get:

The number of moles of is, 6.07 mole

Now we have to calculate the limiting and excess reagent.

From the balanced reaction we conclude that

As, 3 mole of react with 2 mole of

So, 6.07 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of

From the reaction, we conclude that

As, 3 mole of react to give 2 mole of

So, 6.07 moles of react to give moles of

Now we have to calculate the volume of produced at STP.

As, 1 mole of contains 22.4 L volume of

So, 4.05 mole of contains volume of

Therefore, the volume of produced are 90.7 liters.