Heat evolved in the reaction
`H_(2)[g]+Cl_(2)[g] rarr 2HCl[g]` is 182 kJ Bond energies H- H = 430 kJ/mole, `Cl-Cl = 242kJ//"mole"`. The H-Cl bond energy is

Explanation

To find the bond energy of HCl from the given reaction and bond energies, we can follow these steps:

### Step 1: Write the reaction and identify the given data
The reaction is:
\[ H_2(g) + Cl_2(g) \rightarrow 2HCl(g) \]

Given data:
- Heat evolved (ΔH) = -182 kJ (since heat is released, it's negative)
- Bond energy of H-H = 430 kJ/mole
- Bond energy of Cl-Cl = 242 kJ/mole
- Bond energy of HCl = ? (this is what we need to find)

### Step 2: Write the formula for ΔH in terms of bond energies
The change in enthalpy (ΔH) for the reaction can be expressed as:
\[ \Delta H = \text{(Bond energy of reactants)} - \text{(Bond energy of products)} \]

For our reaction:
\[ \Delta H = \text{(Bond energy of H-H) + (Bond energy of Cl-Cl)} - 2 \times \text{(Bond energy of HCl)} \]

### Step 3: Substitute the known values into the equation
Substituting the known bond energies into the equation:
\[ -182 = (430 + 242) - 2 \times \text{(Bond energy of HCl)} \]

### Step 4: Simplify the equation
Calculate the sum of the bond energies of the reactants:
\[ -182 = 672 - 2 \times \text{(Bond energy of HCl)} \]

### Step 5: Rearrange the equation to solve for the bond energy of HCl
Rearranging gives:
\[ 2 \times \text{(Bond energy of HCl)} = 672 + 182 \]
\[ 2 \times \text{(Bond energy of HCl)} = 854 \]
\[ \text{(Bond energy of HCl)} = \frac{854}{2} \]
\[ \text{(Bond energy of HCl)} = 427 \text{ kJ/mole} \]

### Step 6: Final answer
The bond energy of HCl is:
\[ \text{Bond energy of HCl} = 427 \text{ kJ/mole} \]