Please someone help. Urgent Will mark you brainliest

Problem: 0.1156 g CxHyNz reacts with oxygen, O2, to give 0.1638 g CO2, 0.1676 g H2O, and N2. Find the empirical formula of the organic compound.

CxHyNz + O2 → CO2 + H2O + N2

To determine the empirical formula you should know how much carbon, hydrogen, & nitrogen are each present in the sample. Follow the steps: Use dimensional analyses here.

1. Determine how much C is in CO2 then convert to mole.

2. Determine how much H is in H2O then convert to mole.

3. How do you think you can determine the amount of oxygen?

4. How do you think you can determine the amount of nitrogen?

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

5.6⋅10−^19  j

do you need the explaination?