How many grams of ticl4 are needed for complete reaction with 170 l of h2 at 450 ∘c and 785 mm hg pressure?

The answer to your question is 1124.8 g of TiCl₄

Explanation:

Data

TiCl₄ = ?

Volume of H₂ = 170 l

Temperature = 450°C

Pressure = 785 mm Hg

Process

1.- Convert temperature to °K

    Temperature = 273 + 450

    Temperature = 723 °K

2.- Convert mmHg to atm

                 1 atm 760 mmHg

                  x        785 mmHg

                  x = (785 x 1) / 760

                  x = 1.032 atm

3.- Use the Ideal gases law

                   PV = nRT

solve for n

                 n = (PV) / (RT)

Substitution

                 n = (1.032 x 170) / (0.082 x 723)

Simplification

                 n = 175.44 / 59.29

Result

                 n = 2.96 moles of H₂

4.- Use the balanced reaction to calculate the moles of TiCl₄ needed

                    2TiCl₄  +   H₂   ⇒    2TiCl₃  +  HCl

                    2 moles of TiCl₄   1 mol of H₂

                    x                           2,96 mol of H₂

                    x = (2.96 x 2) / 1

                    x = 5.92 moles of TiCl₄

5.- Convert moles to grams

                   190 g of TiCl₄    1 mol of TiCl₄

                     x                     5.92 moles of TiCl₄

                  x = (5.92 x 190) / 1

                  x = 1124.8 g of TiCl₄

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.