Thermochemical equation for the combustion of ethylene gas, `C_(2)H_(4)`, is
`C_(2)H_(4)(g) rarr 2CO_(2)(g) +2H_(2)O(l), DeltaH^(Theta) =- 337 kcal`
Assuming `70%` efficiency, calculate the weight of water at `20^(@)C` that can be converted into system at `100^(@)C` by buring `1m^(3)` of `C_(2)H_(4)` gas measured at `STP`. The heat of vaporisation of water at `20^(@)C` and `100^(@)C` are `1.00 kcal kg^(-1)` and `540 kcal kg^(-1)` respectively.

Explanation

To solve the problem step by step, we will follow the outlined procedure to find the weight of water that can be converted into steam by burning 1 m³ of ethylene gas at 70% efficiency.

### Step 1: Calculate the number of moles of ethylene gas in 1 m³ at STP.

1. **Volume of ethylene gas**: 1 m³ = 1000 liters.
2. **Molar volume at STP**: 22.4 liters/mol.
3. **Number of moles (n)**:
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