Answer:
A. 1.25 moles of C.
B. 0.96 mole of CO.
C. 1 mole of SO2.
D. 0.5 mole of CS2.
Explanation:
We'll begin by writing the balanced equation for the reaction between carbon, C and sulphur (iv) oxide, SO2.
This is given below:
5C + 2SO2 → CS2 + 4CO
From the balanced equation above,
5 moles of C reacted with 2 moles of SO2 to produce 1 mole of CS2 and 4 moles of CO.
A. Determination of the number of moles of C needed to react with 0.5 mole of SO2.
This can be obtained as follow:
From the balanced equation above,
5 moles of C reacted with 2 moles of SO2.
Therefore, Xmol of C will react with 0.5 mole of SO2 i.e
Xmol of C = (5 x 0.5)/2
Xmol of C = 1.25 mole
Therefore, 1.25 moles of C is needed for the reaction.
B. Determination of the number of moles of CO produced when 1.2 moles
of C reacted.
From the balanced equation above,
5 moles of C reacted to 4 moles of CO.
Therefore, 1.2 moles of C will react to produce = (1.2 x 4)/5 = 0.96 mole of CO.
Therefore, 0.96 mole of CO was obtained from the reaction.
C. Determination of the number of moles of SO2 required to produce 0.50 mole of CS2.
This can be obtained as follow:
From the balanced equation above,
2 moles of SO2 reacted to produce 1 mole of CS2.
Therefore, Xmol of SO2 will react to produce 0.5 mole of CS2 i.e
Xmol of SO2 = (2 x 0.5)/1
Xmol of SO2 = 1 mole.
Therefore, 1 mole of SO2 is needed for the reaction.
D. Determination of the number of moles of CS2 produced when 2.5 moles of C reacted.
From the balanced equation above,
5 moles of C reacted to produce 1 mole of CS2.
Therefore, 2.5 moles of C will react to produce = (2.5 x 1)/5 = 0.5 mole of CS2.
Therefore, 0.5 mole of CS2 was produced from the reaction.
