Titanium tetrachloride (TiCl_4) has a molar enthalpy of fusion (ΔH_{fus}) of 9.37 kJ/mol. How much energy is required to melt 261.1 g of TiCl_4?

• A. 9.37 kJ
• B. 35.2 kJ
• C. 141.2 kJ
• D. 24.7 kJ

Answer: (C)

Verified step by step guidance

1. Identify the given data: the molar enthalpy of fusion (\( \Delta H_{fus} \)) of TiCl_4 is 9.37 kJ/mol, and the mass of TiCl_4 to be melted is 261.1 g.
2. Calculate the molar mass of TiCl_4 by summing the atomic masses: Ti (approximately 47.87 g/mol) plus 4 times Cl (approximately 35.45 g/mol each). The formula is \( M = 47.87 + 4 \times 35.45 \).
3. Determine the number of moles of TiCl_4 in 261.1 g using the formula \( n = \frac{\text{mass}}{\text{molar mass}} = \frac{261.1}{M} \).
4. Calculate the total energy required to melt the sample by multiplying the number of moles by the molar enthalpy of fusion: \( q = n \times \Delta H_{fus} \).
5. Express the final answer in kilojoules (kJ), which represents the energy needed to melt 261.1 g of TiCl_4.