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The given chemical equation is:

\[
2 \text{C}_2\text{H}_2 + 5 \text{O}_2 \longrightarrow 4 \text{CO}_2 + 2 \text{H}_2\text{O}
\]

This is a combustion reaction where acetylene (C₂H₂) reacts with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). We are tasked with determining how many grams of oxygen (O₂) are required to completely burn 17 g of acetylene (C₂H₂).

### Step 1: Molar masses
- The molar mass of C₂H₂ (acetylene):  
  \( \text{C} = 12.01 \, \text{g/mol}, \, \text{H} = 1.008 \, \text{g/mol} \)  
  \( \text{C}_2\text{H}_2 = 2(12.01) + 2(1.008) = 26.036 \, \text{g/mol} \)
  
- The molar mass of O₂:  
  \( \text{O}_2 = 2(16.00) = 32.00 \, \text{g/mol} \)

### Step 2: Mole ratio
From the balanced equation, the mole ratio of C₂H₂ to O₂ is:
\[
2 \text{C}_2\text{H}_2 : 5 \text{O}_2
\]
This means 2 moles of acetylene require 5 moles of oxygen.

### Step 3: Calculate moles of acetylene
We are given 17 g of acetylene. First, we calculate how many moles this is:
\[
\text{moles of C}_2\text{H}_2 = \frac{17 \, \text{g}}{26.036 \, \text{g/mol}} \approx 0.653 \, \text{mol}
\]

### Step 4: Determine moles of oxygen needed
Using the mole ratio \( 2 \text{C}_2\text{H}_2 : 5 \text{O}_2 \), we can find how many moles of oxygen are required for 0.653 moles of acetylene:
\[
\text{moles of O}_2 = 0.653 \, \text{mol} \times \frac{5}{2} = 1.633 \, \text{mol}
\]

### Step 5: Convert moles of oxygen to grams
Now, we convert moles of oxygen to grams:
\[
\text{grams of O}_2 = 1.633 \, \text{mol} \times 32.00 \, \text{g/mol} = 52.26 \, \text{g}
\]

Thus, approximately **52 g** of oxygen are required to completely burn 17 g of acetylene.

### Final Answer:
The correct answer is **52 g**.

Would you like further details or have any questions?

Here are 5 related questions to deepen your understanding:
1. How would the required oxygen change if you burned 25 g of acetylene?
2. What is the mass of carbon dioxide produced from burning 17 g of acetylene?
3. How do you calculate the mass of water formed in this reaction?
4. If the oxygen supply is limited to 40 g, how much acetylene can be completely burned?
5. Can you explain the significance of stoichiometric coefficients in balanced equations?

**Tip:** Always start with a balanced chemical equation when solving combustion or any reaction problems, as it provides the necessary mole ratios for stoichiometric calculations.

How many grams of oxygen must be supplied to completely burn 17 g of acetylene according to the balanced combustion reaction?

Learn how to calculate the grams of oxygen required to completely burn 17 g of acetylene using stoichiometry and mole-to-mass conversions. This problem involves key chemistry concepts such as combustion reactions and mole ratios. Suitable for students in Grades 10-12.

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