Answer : The volume of sulfur dioxide measured at STP is, 113.6 L
Explanation :
First we have to calculate the moles of PbS.
Molar mass of PbS = 239.27 g/mol
Now we have to calculate the moles of oxygen gas.
Using ideal gas equation:
where,
P = Pressure of gas = 2.00 atm
V = Volume of gas = 154 L
n = number of moles = ?
R = Gas constant =
T = Temperature of gas =
Putting values in above equation, we get:
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction will be:
From the balanced chemical reaction we conclude that,
As, 3 moles of react with 2 moles of PbS
So, 7.61 moles of react with moles of PbS
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, 7.61 mole of react to give mole of
Now we have to calculate the volume of at STP.
Using ideal gas equation:
where,
P = Pressure of gas = 1.00 atm
V = Volume of gas = ?
n = number of moles = 5.07 mol
R = Gas constant =
T = Temperature of gas = 273 K
Putting values in above equation, we get:
Thus, the volume of sulfur dioxide measured at STP is, 113.6 L