Gaseous ozone is bubbled through water-ice mixture at `0^@C`. As the `O_3(g)` decomposes to form `O_2`(g), the enthalpy of reaction is absorbed by the resulting ice. Given that the heat of fusion of ice is 6.0095 `kJ "mol"^(-1)` , calculate the mass of ice that melts for each gram of `O_3` that decomposes.
`2O_3(g) to 3O_2(g) , Delta H = -285.kJ`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Determine the enthalpy change per mole of O3
The reaction given is:
\[ 2O_3(g) \rightarrow 3O_2(g) \]
with an enthalpy change (\(\Delta H\)) of \(-285 \, \text{kJ}\).

To find the enthalpy change for 1 mole of O3:
...