Question

Carbon disulfide, CS2, can be made from coke, C(s), and sulfur dioxide, SO2(g). C(s) + SO2(g) à CS2(s) + CO2(g) If the actual yield of CS2 is 86.0% of the theoretical yield, what mass of coke is needed to produce 950. grams of CS2?

Answer 1

Answer:

450g of coke (C)

Explanation:

Step 1:

The balanced equation for the reaction is given below:

3C(s) + 2SO2(g) —> CS2(s) + 2CO2(g)

Step 2:

Determination of the mass of C that reacted and the mass of CS2 produced from the balanced equation.

This is illustrated below:

Molar Mass of C = 12g/mol

Mass of C from the balanced equation = 3 x 12 = 36g

Molar Mass of CS2 = 12 + (32x2) = 12 + 64 = 76g/mol.

From the balanced equation above, 36g of C reacted to produce 76g of CS2.

Step 3:

Determination of the mass of C required to produce 950g of CS2. This is illustrated below:

From the balanced equation above, 36g of C reacted to produce 76g of CS2.

Therefore, Xg of C will react to produce 950g of CS2 i.e

Xg of C = (36 x 950)/76

Xg of C = 450g

From the calculations made above, 450g of coke (C) is needed to produce 950g of CS2.