Question

Titanium (III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl4 vapor with H2 :

2TiCl4(g) + H2(g) --> 2TiCl3(s) + 2HCl(g)
a) how many grams of TiCl4 are needed for a complete reaction with 155L of H2 at 435 degrees C and 795 mmHg pressure?
b) How many liters of HCl gas at STP will result from the reaction described in part (a)?

Answer 1

To determine the grams of TiCl4 needed and the volume of HCl gas produced, the ideal gas law and stoichiometry of the reaction are used. First, the moles of H2 are calculated at the given conditions, which in turn provides the moles of TiCl4 needed. The moles of HCl are calculated from the stoichiometry and converted to liters at STP.

Step-by-step explanation:

To solve part a) of the question, we first need to use the ideal gas law to determine the number of moles of H2 gas: PV = nRT. Given that the pressure is 795 mmHg, we convert this to atmospheres as follows: 795 mmHg * (1 atm / 760 mmHg) = 1.046055 atm. For the volume, we have 155 L of H2. We should plug these values into the ideal gas law along with the temperature converted to Kelvin (435 + 273 = 708 K) and the gas constant R (0.0821 L atm mol-1 K-1). This gives us n = PV / (RT).

After calculating the moles of H2, we can then use the stoichiometry of the balanced equation to find out how many moles of TiCl4 are required for a complete reaction, which is a 1:1 mole ratio with H2. We then convert the moles of TiCl4 to grams using its molar mass.

For part b), we use the stoichiometry of the reaction which tells us that 2 moles of HCl are produced for every 2 moles of TiCl4 consumed. Thus, the moles of HCl produced will be the same as the moles of H2 consumed. We then convert the moles of HCl to liters using the standard temperature and pressure (STP) conditions where 1 mole equals 22.4 L.