Find out the heat evolved in combustion if `112` litres ( at `STP`) of water gas (mixture of eqal volume of `H_(2)(g)` and `CO(g)))`. `{:(H_(2)(g)+1//2O_(2)(g)rarrH_(2)O(g),,,,DeltaH= -241.8 kJ),(CO(g)+1//2O_(2)(g)rarrCO_(2)(g),,,,DeltaH= -283 kJ):}`

Explanation

To find out the heat evolved in the combustion of 112 liters of water gas (a mixture of equal volumes of H₂ and CO), we can follow these steps:

### Step 1: Determine the volumes of H₂ and CO
Since the water gas is a mixture of equal volumes of H₂ and CO, and the total volume is 112 liters, we can calculate the volume of each gas.

\[ \text{Volume of } H_2 = \text{Volume of } CO = \frac{112 \text{ liters}}{2} = 56 \text{ liters} \]

### Step 2: Calculate the number of moles of H₂ and CO
Using the ideal gas law, we can find the number of moles of each gas at STP (Standard Temperature and Pressure). At STP, 1 mole of gas occupies 22.4 liters.

\[ \text{Moles of } H_2 = \text{Moles of } CO = \frac{56 \text{ liters}}{22.4 \text{ liters/mole}} = 2.5 \text{ moles} \]

### Step 3: Calculate the heat evolved from the combustion of H₂
The balanced equation for the combustion of hydrogen is:

\[ H_2(g) + \frac{1}{2} O_2(g) \rightarrow H_2O(g) \]

The enthalpy change (ΔH) for this reaction is -241.8 kJ per mole of H₂. Therefore, for 2.5 moles of H₂:

\[ \text{Heat evolved from } H_2 = 2.5 \text{ moles} \times (-241.8 \text{ kJ/mole}) = -604.5 \text{ kJ} \]

### Step 4: Calculate the heat evolved from the combustion of CO
The balanced equation for the combustion of carbon monoxide is:

\[ CO(g) + \frac{1}{2} O_2(g) \rightarrow CO_2(g) \]

The enthalpy change (ΔH) for this reaction is -283 kJ per mole of CO. Therefore, for 2.5 moles of CO:

\[ \text{Heat evolved from } CO = 2.5 \text{ moles} \times (-283 \text{ kJ/mole}) = -707.5 \text{ kJ} \]

### Step 5: Calculate the total heat evolved
To find the total heat evolved from both reactions, we sum the heat evolved from H₂ and CO:

\[ \text{Total heat evolved} = \text{Heat from } H_2 + \text{Heat from } CO \]

\[ \text{Total heat evolved} = -604.5 \text{ kJ} + (-707.5 \text{ kJ}) = -1312 \text{ kJ} \]

### Final Answer
The total heat evolved in the combustion of 112 liters of water gas is **-1312 kJ**.

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