Question

During the naval battles of the South Pacific in World War II, the U.S. Navy produced smoke screens by spraying titanium tetrachloride into the moist air where it reacted according to the equation:

TiCl4 + H2O TiO2 + HCl

a. How many moles of H2O are needed to react with 6.50 moles of TiCl4? (13.0)

b. How many moles of HCl are formed when 8.44 moles of TiCl4 react? (33.8)

Answer 1

Step-by-step explanation:

The reaction given is;

TiCl4 + H2O --> TiO2 + HCl

The reaction is not balanced, upon balancing it is given as;

TiCl4 + 2H2O → TiO2 + 4HCl

a. How many moles of H2O are needed to react with 6.50 moles of TiCl4?

From the reaction;

1 mol of TiCl4 requires 2 mol of H2O

6.50 mol of TiCl4 would require x mol of H2O

1 = 2

6.5 = x

x = 6.5 * 2 / 1 = 13.0 mol

b. How many moles of HCl are formed when 8.44 moles of TiCl4 react?

From the equation of the reaction;

1 mol of TiCl4 reacts to form 4 mol of HCl

8.44 mol of TiCl4 reacts to form x mol of HCl

1 = 4

8.44 = x

x = 8.44 * 4 / 1 = 33.76 mol