Question

C(s) + S8(s) → CS2(l)

How many grams of carbon disulfide will be produced if 7.70 g of C and 19.7 g of S8 are allowed to react completely?

Answer 1

The balanced chemical reaction is written as:

4C(s) + S8(s) → 4CS2(l)

We are given the amount of carbon and sulfur to be used in the reaction. We need to determine first the limiting reactant to be able to solve this correctly.

7.70 g C ( 1 mol / 12.01 g) =0.64 mol C
19.7 g S8 ( 1 mol / 256.48 g) = 0.08 mol S8

The limiting reactant would be S8. We use this amount to calculate.

0.08 mol S8 ( 4 mol CS2 / 1 mol S8 ) ( 256.48 g / 1 mol ) = 78.8 g CS2

Answer 2

If 7.70 gram of C and 19.7 gram of S₈ are allowed to react completely to produce 78.8 g CS₂.

How we convert grams of a substance to moles?

To convert mass of a substance from grams to moles we will use below formula:

n = W / M

Where, W = given mass

M = molar mass

Balanced form of given equation is:

4C(s) + S₈(s) → 4CS₂(l)

Also given that, given mass of carbon = 7.70 g

And given mass of S₈ = 19.7 g

Now we will convert this data in to the mole form by using the above formula:

So, mole of carbon = 7.70 / 12 = 0.64 mol

mole of S₈ = 19.7 / 256 = 0.076 mol

From the above calculation it is clear that S₈  is the limiting reactant, which takes place in the product of product.

Grams of carbon disulfide produced = 0.08 mol S8 ( 4 mol CS2 / 1 mol S8 ) ( 256.48 g / 1 mol ) = 78.8 g CS₂

Hence,  78.8 g of carbon disulfide (CS₂) is produced.

To learn more about mass changes, visit below link:

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