How would you determine the empirical and molecular formula for
hydrogen peroxide, which is 5.94% H and 94.06% O and has a molar mass of 34.01 g/mol?

Question

Noah Aldrich · Accepted Answer

The molecular formula is #"H"_2"O"_2"#.

We can assume that we have a 100-g sample because the percentages add up to 100%. This will enable us to convert the percentages into grams. #"H":##5.94%=>"5.94 g"# #"O":##94.06%=>"94.06 g"# Calculate the Moles of Every Component By dividing the given masses of H and O by their molar masses (atomic weight on the periodic table) in g/mol, we can first calculate the moles of each element. #"H":##5.94cancel"g H"xx(1"mol H")/(1.00794cancel"g H")="5.89 mol H"# #"O":##94.06"g O"xx(1"mol O")/(15.999"g O")="5.88 mol O"# Determine the Empirical Formula and Mole ratios. The mole ratios are 1 because H and O have the same amount of moles. The empirical formula is #"HO"# Find the formula for the molecule. The empirical formula mass is #(1xx1.00794"g/mol")+(1xx15.999"g/mol")="17.007 g/mol"# The molecular formula mass is #"34.01 g/mol"#. To get the multiplication factor, divide the molecular formula mass by the empirical formula mass. #"Multiplication factor"=(34.01"g/mol")/(17.007"g/mol")="2.000"# Multiply the empirical formula's subscripts by two to obtain the molecular formula. The molecular formula is #"H"_2"O"_2"#.

Ellie Andrews · Answer

these formulas are used in solving the problem
n(empirical formula)=molecular formula
n=molecular formula mass/empirical formula mass

Atomic mass of H=1.008 Atomic mass of O=16 amount of hydrogen present in sample=5.94/1.008=5.8 amount of oxygen present in sample=94.06/16=5.8 RATIO: H : O 5.8 : 5.8 1 : 1 so empirical formula= HO n(empirical formula)=molecular formula n=molecular formula mass/empirical formula mass n=34.01/17 =2 2(HO)=H2O2 H2O2 is molecular formula.

Ellie Andrews · Answer

undefined Finding the ratio of the elements present is the first step in determining the empirical formula for hydrogen peroxide. Based on the provided percentages, assume that you have 100 g of the compound. Next, find the simplest whole-number ratio of the elements. The empirical formula for hydrogen peroxide is HO. Next, find the molecular formula by calculating the number of moles of each element using its molar mass. Since the molar mass of hydrogen peroxide is close to the molar mass of the empirical formula, the molecular formula is also HO.

How would you determine the empirical and molecular formula for hydrogen peroxide, which is 5.94% H and 94.06% O and has a molar mass of 34.01 g/mol?