Question

An inorganic compound contains 5.88% of hydrogen and 94.11% oxygen. Find out the empirical formula of the compound and predict the molecular formula.

• A. $H_{2}O$
• B. $HO$
• C. $H_3{O}_2$
• D. $H_5{O}_2$

Answer 1

The correct option is B $HO$

With all these empirical formula problems, we assume that there are 100 g of

an unknown compound, and work out the empirical formula appropriately:

mole of hydrogen = $\frac{5.88g}{1\left(g/mol\right)}$ = 5.88mol

mole of oxygen = $\frac{94.11\left(g\right)}{16\left(g/mol\right)}$ = 5.88 mol

hydrogen and oxygen moles ration is equal to one hence answer is $HO$

answer is B