In an experiment, 0.6mol of chlorine gas, Cl2, is reacted with an excess of hot aqueous sodium hydroxide. One of the products is a compound of sodium, oxygen and chlorine. Which mass of this product is formed?

A 21.3 B 44.7 C 63.9 D 128

Answer: B) 44.7 g

Explanation:

The equation represent the reaction is

Cl2 + 2NaOH → NaCl + NaClO + H2O

The balanced equation shows that every mole of Cl2 reacts to produce mole of NaClO

0.6 mole of Cl2 will produce 0.6 mole of NaClO

n = mass/molar mass

molar mass of NaClO = 74.5 g/mol

the mass of NaClO = n x molar mass = (0.6 mole) (74.5 g/mol) = 44.7 g