Carbon disulfide is an important industrial solvent. It is prepared by the reaction of carbon (called coke) with sulfur dioxide. Carbon monoxide is also produced (as a byproduct) of this reaction. (a) Write the equation that correctly demonstrates this reaction and balance it. (b) How many moles of carbon are needed to produce 45.90 moles of carbon disulfide?

Question

Chemistry

Ricardo Hansen

2 October, 06:37

Carbon disulfide is an important industrial solvent. It is prepared by the reaction of carbon (called coke) with sulfur dioxide. Carbon monoxide is also produced (as a byproduct) of this reaction. (a) Write the equation that correctly demonstrates this reaction and balance it. (b) How many moles of carbon are needed to produce 45.90 moles of carbon disulfide?

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Answers (1)

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Danna Harper · Answer 1

A. The balanced equation is given below:

5C + 2SO2 - > CS2 + 4CO

B. 229.5 moles of carbon.

Explanation:

A. Step 1:

The equation for the reaction is given below:

C + SO2 - > CS2 + CO

A. Step 2:

Balancing the equation.

The above equation can be balanced as follow:

There are 2 atoms of S on the right side and 1 atom on the left side. It can be balance by putting 2 in front of SO2 as shown below:

C + 2SO2 - > CS2 + CO

There are 4 atoms of O on the left side and 1 on the right. It can be balance by putting 4 in front of CO as shown below:

C + 2SO2 - > CS2 + 4CO

There are a total of 5 atoms of C on the right side and 1 atom on the left. It can be balance by putting 5 in front of C as shown below:

5C + 2SO2 - > CS2 + 4CO

Now the equation is balanced

B. Determination of the number of moles of carbon needed to produce 45.90 moles of carbon disulfide.

This is illustrated below:

5C + 2SO2 - > CS2 + 4CO

From the balanced equation above,

5 moles of C produced 1 mole of CS2.

Therefore, Xmol of C will produce 45.90 moles of CS2 i. e

Xmol of C = 5 x 45.90

Xmol of C = 229.5 moles

229.5 moles of carbon is needed to produce 45.90 moles of carbon disulfide.