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(b) H(2)O(l) to H(2)O(s), Delta(r)H^(@) ...

(b) `H_(2)O(l) to H_(2)O(s), Delta_(r)H^(@) = -6.01 kJ`
`DeltaH` is the heat of ........of water.

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To solve the question, we need to understand the process described by the given enthalpy change, ΔH. The notation provided indicates a transition from liquid water (H₂O(l)) to solid water (H₂O(s)), with a given enthalpy change of ΔH = -6.01 kJ. ### Step-by-Step Solution: 1. **Identify the Process**: The transition from liquid water to solid water is known as freezing or solidification. In this process, water loses heat to form ice. 2. **Understand the Sign of ΔH**: The negative sign in ΔH = -6.01 kJ indicates that the process is exothermic. This means that heat is released when liquid water freezes to form solid water. ...
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