7. A compound has the empirical formula CH and a molar mass of 78.11 g/mol. What is its molecular formula?
8. Upon combustion, a compound containing only carbon and hydrogen produces 1.83 g CO2 and 0.901 g H2O. Find the empirical formula of the compound.
9. Write a balanced equation for the reaction between solid cobalt(III) oxide and solid carbon to produce solid cobalt and carbon dioxide gas.
7)
molar mass = 78.11 g/mol
emperical formula = CH
emperical formula mass = 12 + 1 = 13 g/mol
n = molar mass / emperical formula mass
= 78.11 / 13
= 5.85
= 6
molecular formula = C6H6
8)
moles of CO2 = 1.83 / 44 = 0.0416
moles of C =0.0416
moles of H2O = 0.901 / 18 = 0.05
moles of H = 0.100
C H
0.0416 0.100
1 2.5
emperical formula = C2H5
Get Answers For Free
Most questions answered within 1 hours.