Question

Methane and sulfur react to produce carbon disulfide (CS2), a liquid often used in the production of cellophane.
CH4(g) + S8(s) CS2(l) + H2S(g)
(a) Balance the equation. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)
(b) Calculate the moles CS2 produced when 2.12 mol S8 is used.
(c) How many moles H2S are produced?

Answer 1

Answer:

a) 2CH4(g) + S8(s) → 2CS2(l) + 4H2S(g)

b) 4.24 moles CS2

c) 8.48 moles H2S

Explanation:

Step 1: The unbalanced equation

CH4(g) + S8(s) → CS2(l) + H2S(g)

(a) Balance the equation. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answe.)

2CH4(g) + S8(s) → 2CS2(l) + 4H2S(g)

(b) Calculate the moles CS2 produced when 2.12 mol S8 is used.

For 2 moles CH4 we need 1 mol S8 to produce 2 moles CS2 and 4 moles H2S

For 2.12 moles S8 we'll have 2*2.12 = 4.24 moles CS2

(c) How many moles H2S are produced?

For 2 moles CH4 we need 1 mol S8 to produce 2 moles CS2 and 4 moles H2S

For 2.12 moles S8 we'll have 4*2.12 = 8.48 moles H2S

Answer 2

a) $2CH_4(g) + S_8(s)$ → $2CS_2(l) + 4H_2S(g)$

b) 4.24 moles of  CS₂

c) 8.48 moles of  H₂S

Let's solve each part one by one:

(a) Balance the equation.

We need to balance the chemical equation first:

$2CH_4(g) + S_8(s)$ → $2CS_2(l) + 4H_2S(g)$

(b) Calculate the moles CS₂ produced when 2.12 mol S₈ is used.

2 moles of  CH₄  and 1 mol of S₈ are required to produce 2 moles of CS₂.

Thus,

For 2.12 moles S₈,

The moles for CS₂ will be  2*2.12 = 4.24 moles

(c) How many moles H₂S are produced?

2 moles of  CH₄  and 1 mol of S₈ are required to produce 4 moles of H₂S.

For 2.12 moles S₈,

The moles for H₂S will be 4*2.12 = 8.48 moles

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