Question

Tungsten metal reacts with chlorine to form a compound (containing only W and Cl) used in the production of filaments in incandescent light bulbs. 3.6768 g of W is reacted with excess chlorine gas and produces 7.930 grams of the material.

A. Determine the formula of the compound

B. Name the compound

C. Determine the molar mass of the compound

D. Write a balanced equation for the formation of the compound from W and Cl2 gas

E. Determine the amount of chlorine gas in grams required to react with the initial amount of W metal

Answer 1

W + n Cl₂ -----------> WCl_n

molar mass 183.84 71 ?

A. 3.6768 g of W reacts with Cl2 to give 7.930 g of WCln comple. What is the n= ?

183.84 g (molar mass) of W gives how much WCln ?

wt of WCln or (molar mass of WCln) = 183.84 *7.930 / 3.6768 = 396.5 g

The WCLn molar mass is 396.5 g. That means [183.84 + n (35.5)] = 396.5 g

n = no of Cl atoms = 6

The compound is WCl₆

B. Tungsten hexachloride or Tungsten(VI) chloride

c. The molar mass of the WCl₆ ​- 183.84 + 6*35.5 = 396.5

d.   W + 3 Cl₂ -----------> WCl₆

e. 183.84 g of W reacts with  213 g of Cl2 (3*71 g) to give 396.5 g of WCl6 comple.

3.6768 g of W needs how much Cl2  ?

= 3.6768 *213/ 183.84 = 4.26 g

the amount of chlorine gas in grams required to react with the initial amount of W metal is 4.26 g