Which of the following represents the correct increasing order of volume of oxygen required per mole for complete combustion under the same conditions?

Options

A. Propyne `lt` Ethyne `lt` Ethane `lt` Ethene
B. Ethyne `lt` Ethenes `lt` Ethane `lt` Propyne
C. Ethene `lt` Ethyne `lt` Ethane `lt` Propyne
D. Ethyne `lt` Ethane `lt` Ethene `lt` Propyne

Explanation

To determine the correct increasing order of the volume of oxygen required per mole for complete combustion of different hydrocarbons, we will analyze the combustion reactions of ethane, ethylene, acetylene, and propane.

### Step-by-Step Solution:

1. **Identify the Hydrocarbons**:
- Ethane (C2H6)
- Ethylene (C2H4)
- Acetylene (C2H2)
- Propane (C3H8)

2. **Write the Combustion Reactions**:
- **Ethane (C2H6)**:
\[ C2H6 + \frac{7}{2} O2 \rightarrow 2 CO2 + 3 H2O \]
For 1 mole of ethane, oxygen required = \(\frac{7}{2}\) moles.

- **Ethylene (C2H4)**:
\[ C2H4 + 3 O2 \rightarrow 2 CO2 + 2 H2O \]
For 1 mole of ethylene, oxygen required = 3 moles.

- **Acetylene (C2H2)**:
\[ C2H2 + \frac{5}{2} O2 \rightarrow 2 CO2 + H2O \]
For 1 mole of acetylene, oxygen required = \(\frac{5}{2}\) moles.

- **Propane (C3H8)**:
\[ C3H8 + 5 O2 \rightarrow 3 CO2 + 4 H2O \]
For 1 mole of propane, oxygen required = 5 moles.

3. **Calculate the Volume of Oxygen Required**:
- At STP, 1 mole of gas occupies 22.4 liters.
- **Ethane**:
\[ \frac{7}{2} \times 22.4 = 78.4 \text{ liters} \]
- **Ethylene**:
\[ 3 \times 22.4 = 67.2 \text{ liters} \]
- **Acetylene**:
\[ \frac{5}{2} \times 22.4 = 56 \text{ liters} \]
- **Propane**:
\[ 5 \times 22.4 = 112 \text{ liters} \]

4. **Determine the Increasing Order**:
- Acetylene (56 liters)
- Ethylene (67.2 liters)
- Ethane (78.4 liters)
- Propane (112 liters)

Thus, the correct increasing order of the volume of oxygen required per mole for complete combustion is:
**Acetylene < Ethylene < Ethane < Propane**.

### Final Answer:
Acetylene < Ethylene < Ethane < Propane

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