Acompound of nitrogen and oxygen is 30.46 percent by mass of n and 69.54 percent by mass o. the molar mass if the compound was determined to be 92g/mol. what is the emperical formula and molecular formular

Empirical formula is and molecular formula is

Explanation: To find the empirical and molecular formula, we follow few steps:

Step 1: Converting mass percent into mass

We are given the percentage of elements by mass. So, the total mass take will be 100 grams.

Therefore, mass of nitrogen =

Similarly, mass of oxygen =

Step 2: Converting the masses into their respective moles

We use the formula:

Molar mass of Nitrogen = 14 g/mol

Molar mass of oxygen = 16 g/mol

Moles of nitrogen =

Moles of oxygen =

Step 3: Getting the mole ratio of nitrogen and oxygen by dividing the calculated moles by the lowest mole value.

Mole ratio of nitrogen =

Mole ratio of oxyegn =

Step 4: The mole ratio of elements are represented as the subscripts in a empirical formula, we get

Empirical formula =

Step 5: For molecular formula, we divide the molar mass of the compound by the empirical molar mass.

Empirical molar mass of

Empirical molar mass = 46 g/mol

Molar mass of the compound = 92 g/mol

Now, multiplying each of the subscript of empirical formula by 'n', we get

Molecular formula =

more info ? ? i don't understand what the question is

explanation:

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.