The gaseous hydrocarbon acetylene, $$ \mathrm{C}_{2} \mathrm{H}_{2} $$, used in welders' torches, burns according to the following equation: $$ 2 \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ Express your answer with the appropriate units.

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To solve the problem, we need to analyze the combustion reaction of acetylene ($$ \mathrm{C}_{2} \mathrm{H}_{2} $$) and determine the stoichiometric relationships between the reactants and products.

The balanced chemical equation is:

$$
2 \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g}) + 5 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{g}) + 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$

### Step 1: Identify the stoichiometric coefficients
From the balanced equation, we can see the following stoichiometric relationships:
- 2 moles of $$ \mathrm{C}_{2} \mathrm{H}_{2} $$ react with 5 moles of $$ \mathrm{O}_{2} $$.
- This reaction produces 4 moles of $$ \mathrm{CO}_{2} $$ and 2 moles of $$ \mathrm{H}_{2} \mathrm{O} $$.

### Step 2: Determine the amount of reactants and products
If we know the amount of one of the reactants or products, we can calculate the amounts of the others using the stoichiometric coefficients.

For example, if we start with 2 moles of $$ \mathrm{C}_{2} \mathrm{H}_{2} $$:
- It will require $$ 5 $$ moles of $$ \mathrm{O}_{2} $$.
- It will produce $$ 4 $$ moles of $$ \mathrm{CO}_{2} $$ and $$ 2 $$ moles of $$ \mathrm{H}_{2} \mathrm{O} $$.

### Step 3: Calculate the amounts based on a given quantity
If you have a specific quantity of $$ \mathrm{C}_{2} \mathrm{H}_{2} $$ or $$ \mathrm{O}_{2} $$, you can use the stoichiometric ratios to find the amounts of the other substances involved.

For example, if you start with 1 mole of $$ \mathrm{C}_{2} \mathrm{H}_{2} $$:
- The amount of $$ \mathrm{O}_{2} $$ needed would be calculated as follows:

$$
\text{Moles of } \mathrm{O}_{2} = \left( \frac{5 \text{ moles of } \mathrm{O}_{2}}{2 \text{ moles of } \mathrm{C}_{2} \mathrm{H}_{2}} \right) \times 1 \text{ mole of } \mathrm{C}_{2} \mathrm{H}_{2} = 2.5 \text{ moles of } \mathrm{O}_{2}
$$

- The amount of $$ \mathrm{CO}_{2} $$ produced would be:

$$
\text{Moles of } \mathrm{CO}_{2} = \left( \frac{4 \text{ moles of } \mathrm{CO}_{2}}{2 \text{ moles of } \mathrm{C}_{2} \mathrm{H}_{2}} \right) \times 1 \text{ mole of } \mathrm{C}_{2} \mathrm{H}_{2} = 2 \text{ moles of } \mathrm{CO}_{2}
$$

- The amount of $$ \mathrm{H}_{2} \mathrm{O} $$ produced would be:

$$
\text{Moles of } \mathrm{H}_{2} \mathrm{O} = \left( \frac{2 \text{ moles of } \mathrm{H}_{2} \mathrm{O}}{2 \text{ moles of } \mathrm{C}_{2} \mathrm{H}_{2}} \right) \times 1 \text{ mole of } \mathrm{C}_{2} \mathrm{H}_{2} = 1 \text{ mole of } \mathrm{H}_{2} \mathrm{O}
$$

### Conclusion
If you provide a specific quantity of $$ \mathrm{C}_{2} \mathrm{H}_{2} $$ or $$ \mathrm{O}_{2} $$, I can calculate the exact amounts of the other reactants and products based on that quantity. Please specify the amount you would like to use for the calculations.
To determine the amounts of reactants and products in the combustion of acetylene ($$ \mathrm{C}_{2} \mathrm{H}_{2} $$), use the balanced equation: $$ 2 \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g}) + 5 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{g}) + 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ For example, 2 moles of $$ \mathrm{C}_{2} \mathrm{H}_{2} $$ react with 5 moles of $$ \mathrm{O}_{2} $$ to produce 4 moles of $$ \mathrm{CO}_{2} $$ and 2 moles of $$ \mathrm{H}_{2} \mathrm{O} $$.

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