Reaction of titanium and chlorine at 300 °C yields a metal halide that is 25.25% Ti by mass. The melting point (124 °C) and boiling point (136 °C) of the halide suggest it is a molecular compound rather than an ionic one. (a) What are the formula and name of the compound, assuming the molecular formula is the same as the empirical formula? (b) Write the balanced equation for the reaction.

Verified step by step guidance

1. Step 1: Determine the empirical formula of the compound. Assume 100 g of the compound, which means it contains 25.25 g of Ti. Calculate the moles of Ti using its molar mass (47.87 g/mol).
2. Step 2: Calculate the mass of chlorine in the compound by subtracting the mass of titanium from the total mass (100 g - 25.25 g = 74.75 g of Cl). Then, calculate the moles of Cl using its molar mass (35.45 g/mol).
3. Step 3: Determine the simplest whole number ratio of moles of Ti to moles of Cl to find the empirical formula. Divide the moles of each element by the smallest number of moles calculated.
4. Step 4: Since the problem states that the molecular formula is the same as the empirical formula, use the empirical formula as the molecular formula. Name the compound based on its formula.
5. Step 5: Write the balanced chemical equation for the reaction of titanium with chlorine gas to form the compound. Use the stoichiometry of the reaction to ensure the equation is balanced.