Acetylene burns in air according to the reaction `2C_(2)H_(2) + 5O_(2) to4CO_(2) + 2H_(2)O` at 100°C. Calculate the volume of air required to completely burn 50 cc of acetylene. (Air contains 20% oxygen by volume).

Explanation

To solve the problem of calculating the volume of air required to completely burn 50 cc of acetylene (C₂H₂), we will follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the combustion of acetylene is:
\[ 2C_{2}H_{2} + 5O_{2} \rightarrow 4CO_{2} + 2H_{2}O \]

### Step 2: Determine the volume of oxygen required
From the balanced equation, we see that 2 moles of acetylene require 5 moles of oxygen. Therefore, the volume of oxygen required can be calculated using the ratio from the equation.
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