During the first stage of the Contact Process for the industrial manufacture of tetraoxosu… — JAMB UTME

During the first stage of the Contact Process for the industrial manufacture of tetraoxosulfate(VI) acid, pure sulfur is burned in dry air to produce sulfur(IV) oxide gas according to the equation:

S(s) + O_2(g) \rightarrow SO_2(g)

What volume of sulfur(IV) oxide gas, in

\text{dm}^3

measured at standard temperature and pressure (STP), is produced by the complete combustion of

16.0\text{ g}

of sulfur?
[Relative atomic mass:

S = 32

; Molar volume of gas at STP =

22.4\text{ dm}^3\text{ mol}^{-1}

]

Answer: 11.2 dm³

Answer

The volume of sulfur(IV) oxide gas produced at STP is

11.2\text{ dm}^3

According to the balanced equation

S(s) + O_2(g) \rightarrow SO_2(g)

1\text{ mol}

(

32\text{ g}

) of sulfur yields

1\text{ mol}

(

22.4\text{ dm}^3

at STP) of sulfur(IV) oxide gas. Therefore,

16.0\text{ g}

of sulfur corresponds to

\frac{16.0}{32} = 0.50\text{ mol}

, which produces

0.50 \times 22.4\text{ dm}^3 = 11.2\text{ dm}^3

SO_2

gas at STP.

Step-by-Step Solution

Calculate the amount in moles of sulfur reacted.

0.50\text{ mol}

of sulfur.

Using the formula

\text{moles} = \frac{\text{mass}}{\text{molar mass}} = \frac{16.0\text{ g}}{32.0\text{ g mol}^{-1}} = 0.50\text{ mol}

Use the mole ratio from the balanced chemical equation to find moles of sulfur(IV) oxide gas formed.

0.50\text{ mol}

SO_2(g)

The equation shows a 1:1 stoichiometric ratio between

S(s)

and

SO_2(g)

Calculate the gas volume at standard temperature and pressure (STP).

11.2\text{ dm}^3

Multiply the moles of gas by the molar volume at STP:

V = 0.50\text{ mol} \times 22.4\text{ dm}^3\text{ mol}^{-1} = 11.2\text{ dm}^3

Key Concept

Stoichiometric Volume Calculations for Gas Generation in the Contact Process

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