Question

(typed answer please)

Calculate the volume, at 20°C and 1.00 atm, of SO₂ produced by the conventional roasting of 1.00 tonnes (1,000 kg) of nickel sulfide ore, NiS. What mass of pure sulfuric acid could be produced from this amount of SO₂?

Answer 1

Given data

mass of NiS = 1000kg

(1kg = 1000g)

mass of NiS = 1000×1000g

mass of NiS = 106g

We know that, molar mass of NiS = 90.76g/mol

Molar mass of SO​​​​​2 = 64.066g/mol

Step (1) Calculation for Mass of SO2

Balance chemical reaction will be given as follows

2NiS + 3O​​​​​​2  -----------------> 2NiO + 2SO2

From the stoichiometric of balance chemical equation

2mol NiS produced 2 mol of SO​​​​​2

Or

1mol NiS produced 1 mol of SO​​​​​2

Or

90.76g NiS (i,e Mass of 1mol NiS) produced 64.066g SO​​​​​2 (i,e Mass of 1mol SO​​​​​2)

So

1g NiS produced (64.066/90.76)g SO​​​​​2

So,

106g NiS produced (64.066/90.76)×106g SO​​​​​2

Mass of SO​​​​​2 = (64.066/90.76)×106g

Mass of SO​​​​​2 = 705.88×103g

Mass of SO​​​​​2 = 705.88kg

step(2) Calculation for number of mole of SO​​​​​2

Number of mole = Mass /molar mass

Number of Mole of SO​​​​​2

n = 705.88×103g/(64.066g/mol)

n = 11.018×103mol

Step(3) Calculation for volume of SO​​​​​2

we know that, ideal fasa equation is.

PV = nRT .........(1)

Or

V = nRT/P ..........(2)

Where,

V = VOLUME OF GAS

n = Number of mole of gass = 11.018×103mol

R = gas constant = 0.082L.atm/mol.K

T = Temperature = 20°C = (20+273)K = 293K

P = pressure = 1.0atm

Putting the all value in equation number (2)

V=(11.018×103mol)(0.082L.atm/mol.K)(293K)/(1.0atm)

V = 2.65×105L