Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl₄ vapor with H₂: 2 TiCl₄(g) + H₂(g) → 2 TiCl₃(s) + 2 HCl(g) (a) How many grams of TiCl₄ are needed for complete reaction with 155 L of H₂ at 435 °C and 795 mm Hg pressure?

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Convert the pressure from mm Hg to atm using the conversion factor: 1 atm = 760 mm Hg.

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Use the ideal gas law, PV = nRT, to calculate the number of moles of H2. Here, P is the pressure in atm, V is the volume in liters, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.

Use the stoichiometry of the balanced chemical equation to find the moles of TiCl4 needed. According to the equation, 2 moles of TiCl4 react with 1 mole of H2.

Calculate the mass of TiCl4 required using its molar mass. Multiply the moles of TiCl4 by its molar mass to find the grams needed.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the number of moles of hydrogen gas (H2) in the given conditions of temperature and pressure, allowing us to determine how much titanium(IV) chloride (TiCl4) is needed for the reaction.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. In this case, the balanced equation shows that 2 moles of TiCl4 react with 1 mole of H2, which is crucial for determining the amount of TiCl4 required once the moles of H2 are known.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). To find the grams of TiCl4 needed, we must first calculate its molar mass and then use the stoichiometric ratios from the balanced equation to convert moles of TiCl4 into grams, ensuring the complete reaction with the available H2.

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