Calculate the entropy change in surroundings when 1.00 mole of `H_2O(l)` is formed under standard conditions.
`Delta_fH^@ = -286 kJ mol^(-1)`

Explanation

To calculate the entropy change in the surroundings when 1.00 mole of \( H_2O(l) \) is formed under standard conditions, we will follow these steps:

### Step 1: Understand the Given Data
We are given the standard enthalpy of formation (\( \Delta_fH^\circ \)) of \( H_2O(l) \) as -286 kJ/mol. This indicates that the formation of water from its elements is an exothermic reaction, meaning heat is released to the surroundings.

### Step 2: Determine the Heat Released
Since the formation of 1 mole of \( H_2O(l) \) is exothermic, the heat released to the surroundings is equal to the negative of the enthalpy change:
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