Hydrogen sulfide gas gives rotten eggs their terrible odor. hydrogen sulfide burns in air (o2) to produce sulfide dioxide gas and water vapor. in 1.38 moles of sulfide dioxide are produced when this reaction occurs, how many moles of oxygen were required?

2.07 mol O₂

Explanation:

First we need to write down the species present in the chemical equation, using the information given by the exercise:

However this equation is not balanced, so now we balance it:

Now we can use the stoichiometric ratio to calculate the moles of oxygen from the moles of sulfide dioxide:

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.