Question

The white pigment TiO2 is prepared by the reaction of titanium tetrachloride, TiCl4, with water vapor in the gas phase. TiCl4(g) + 2H2O(g)TiO2(s) + 4HCl(g) How much heat is involved in the production of exactly 3.15 mol of TiO2(s) under standard state conditions?

Answer 1

TiCl4(g) + 2H2O(g)------------->TiO2(s) + 4HCl(g)   

Hrxn   = H⁰f products - H⁰f reactans

             = 4*-92-945 -(-763+2*-241.82)

               = -66.36KJ/mole

The heat energy released to production of 1 mole of TiO2 = -66.36KJ

The heat energy released to production of 3.15 moles of TiO2 = -66.36*3.15/1   = -209.034 KJ