Final answer:
The energy required to melt 263.1 g of TiCl₄ cannot be calculated without the specific enthalpy of fusion for TiCl₄. As a reference, melting 2.00 kg of ice requires 334 kJ of energy with water's known enthalpy of fusion.
Step-by-step explanation:
To determine how much energy is required to melt 263.1 g of titanium tetrachloride (TiCl₄), we need specific information, such as the enthalpy of fusion for TiCl₄, which is not provided in the question or the reference information. Typically, this information would be found in a chemical database or a chemistry textbook. Without this critical piece of data, it is impossible to provide an accurate amount of energy required for melting the given mass of TiCl₄.
For example, if we had the enthalpy of fusion for TiCl₄, we could calculate the energy required using the formula: Energy = mass x enthalpy of fusion. Since we don't have this data for TiCl₄, we can look to a similar practice problem that provides an answer for the melting of ice. The practice problem states that melting 2.00 kg of ice at 0 °C requires 334 kJ of energy.
Again, keep in mind that without the specific heat of fusion for TiCl₄, the calculation for the energy required to melt 263.1 g of TiCl₄ cannot be completed.