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Title: How do yu write a balanced equation of the combustion of this compound? Post by: tonio613 on Nov 12, 2012 Combustion of 8.652g of a compound containing C, H, O, and N yields 11.088g of CO2 3.780g of H2O and 3.864g of NO2
Title: How do yu write a balanced equation of the combustion of this compound? Post by: nxstudent on Nov 12, 2012 this is not an equation question I think itis an empirical formula question
here is the solution mass of CO2 =11.088g moles of CO2 =0.252moles moles of C =0.252moles mass of C =3.024g mass of water =3.78g moles of water =0.21moles moles of H =0.42moles mass of H0.42336g mass of NO2 =3.864g moles of NO2 =0.084moles moles of N =0.084moles mass of N =1.176g if we assume the compound is C, H and N only we get the O by difference mass of compound 8.652g mass of O4.02864g moles of O0.33572moles our moles are C0.252 H0.42 N0.084 O0.33572 or dividing by the smallest C3 H5 N1 O3.996666667 empirical formula is C3H5NO4 we don't know if this is the molecular formula but if it was we could write a combustion equation 2C3H5NO4 + 9O2 => 6CO2 +5H2O + 2NO2 Title: How do yu write a balanced equation of the combustion of this compound? Post by: ilovebio123 on Nov 12, 2012 So you get:
4 C3H5NO4 + 13 O2 --> 12 CO2 + 10 H2O + 4 NO2 |