The problem asks for the volume of carbon tetrachloride gas produced when 5.7 L of methane gas are consumed in a reaction between methane and chlorine gas, forming hydrogen chloride and carbon tetrachloride.

Step 1: Write the balanced chemical equation.

The reaction is: $\text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g)$

This shows that for every 1 mole (or volume) of methane (CH₄), 1 mole (or volume) of carbon tetrachloride (CCl₄) is produced.

Step 2: Apply the molar ratio.

Since the volume of gases at constant temperature and pressure is proportional to the number of moles, the volume ratio of CH₄ to CCl₄ is 1:1. Therefore, the volume of carbon tetrachloride produced is the same as the volume of methane consumed.

Given that 5.7 L of methane is consumed, the same volume of carbon tetrachloride will be produced.

Step 3: Answer with correct significant digits.

Since the volume of methane is given to two significant digits (5.7 L), the answer should also be reported to two significant digits.

Thus, the volume of carbon tetrachloride produced is: $\boxed{5.7 \, \text{L}}$

Would you like a more detailed explanation or have any other questions?

Related questions:

1. What is the role of chlorine gas in this reaction?
2. How do you balance chemical equations involving gases?
3. What are the properties of carbon tetrachloride?
4. How would the result change if only 2.5 L of methane were consumed?
5. Can this reaction be reversed under normal conditions?

Tip:

Always check the stoichiometric ratios between reactants and products in a balanced chemical equation to ensure accurate calculations.