Question

I have a chemistry writing promp but it’s asking questions here the prompt: What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen? State three potential molecular formulas from the empirical formula in A. If the molecular formula mass in A is 760 grams/mol, what is the molecular formula? WIll the molecular and empirical formulas in A and D have the same characteristics? Why or why not?

Answer 1

Step-by-step explanation:

1. Find the empirical formula of a compound that has 36.84% of Nitrogen (N), 63.16% of Oxygen (O).

Secondly, Find molar mass of each component: N=14.0067, O=15.9994

Thirdly, convert to moles: N=2.6301698472874, O=3.9476480368014

Then find smallest mole value: 2.6301698472874

Divide all components my smallest value: N=1, O=1.5009099282591

Then divide by fractional component of each mole value: N=1.9963668986866, O=2.9963668986866

Round to closest whole numbers: N=2, O=3

Lastly, combine to get the empirical formula:N2O3