Question

compound the percentage of hydrogen is 5.9 % and oxygen is 94.1 person molecular mass of compound is 34 AMU calculate is molecular formula

Answer 1

We are given that the percentage of oxygen and hydrogen in the given compound is 94.1 and 5.9 respectively. Thus 100g of the compound will contain 94.1g of oxygen and 5.9g of hydrogen. 

Therefore number of moles in 94.1g of oxygen = mass of oxygen / molar mass of oxygen  = 94.1 / 16 = 5.881

Similarly number of moles in 5.9g of hydrogen = mass of hydrogen /  molar mass of hydrogen =  5.9 / 1.008 =  5.853

For expressing the simplest ratio of the elements, we will divide the number of moles of each element by the smallest number that is 5.853. 

Oxygen = 5.881 / 5.853 = 1.005 ≈ 1

Hydrogen =  5.853 / 5.853 = 1

So the empirical formula is OH. Now we are given that the molecular mass is 34 u. So in order to calculate the molecular mass by empirical mass. Thus we get

n = molecular mass / empirical mass

where n is the factor by which the empirical formula should be multiplied in order to obtain the correct molecular formula. So 

n = 34 / (atomic mass of oxygen + atomic mass of hydrogen)

 = 34 / (16 + 1)

 = 34 / 17 = 2

Thus the molecular formula is (OH)n = (OH)2= H2O2

Answer 2

Answer:

Solve in this way u will get it