Question

Lead can be prepared from galena [lead(II) sulfide] by first roasting the galena in oxygen gas to form lead(II) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide.
(a) Write a balanced equation for each step, including the state of each chemical.

(1)

(2)

(b) Write an overall balanced equation for the process, including the state of each chemical.

Answer 1

Answer:

a) Step 1:

$2PbS(g)+3O_2(g)\overset{roasting}\rightarrow 2PbO(s)+2SO_2(g)$

Step 2:

$2PbO(s)+PbS(s)\overset{\Delta }\rightarrow 3Pb(l)+SO_2(g)$

b) The overall balanced reaction for given process is ;

$3PbS(s)+3O_2(g)\rightarrow 3Pb(l)+3SO_2(g)$

Explanation:

a)

Galena = $PbS$

Lead(II) oxide = $PbO$

Sulfur dioxide = $SO_2$

Step 1:

Roasting the galena in oxygen gas to form lead(II) oxide and sulfur dioxide.

Balanced equation of step 1:

$2PbS(g)+3O_2(g)\overset{roasting}\rightarrow 2PbO(s)+2SO_2(g)$..[1]

Step 2:

Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide.

Balanced equation of step 2:

$2PbO(s)+PbS(s)\overset{\Delta }\rightarrow 3Pb(l)+SO_2(g)$..[2]

b)

For over all reaction add [1] and [2]. The overall balanced reaction for given process is ;

$3PbS(s)+3O_2(g)\rightarrow 3Pb(l)+3SO_2(g)$

Answer 2

Answer:

b

Explanation: