The 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, we will follow these steps:

### Step 1: Calculate the number of moles of C₂H₄ in 1 m³ at STP
At STP (Standard Temperature and Pressure), 1 mole of gas occupies 22.4 liters. Therefore, to find the number of moles in 1 m³ (1000 liters):

\[ \text{Number of moles} = \frac{1000 \text{ L}}{22.4 \text{ L/mol}} \approx 44.64 \text{ moles} \]
...