What is the amount of heat released when 35.0 g of H_2O freezes at 0^ext{o}C? (The enthalpy of fusion for water is 334 J/g.)

• A. 117 J
• B. 334 J
• C. 11,690 J
• D. 1,170 J

Answer: (C)

Verified step by step guidance

1. Identify the process: freezing of water at 0°C, which is the reverse of melting (fusion). Since freezing releases heat, the enthalpy change will be negative of the enthalpy of fusion.
2. Write down the given data: mass of water, \(m = 35.0\ \text{g}\), and enthalpy of fusion, \(\Delta H_{fusion} = 334\ \text{J/g}\).
3. Calculate the total heat released using the formula \(q = m \times \Delta H\), where \(\Delta H\) is the enthalpy change per gram. Since freezing releases heat, use \(\Delta H = -334\ \text{J/g}\).
4. Substitute the values into the formula: \(q = 35.0\ \text{g} \times (-334\ \text{J/g})\).
5. Perform the multiplication to find the amount of heat released (note: do not calculate the final number here, just set up the expression).