Question #24794

a. If 4.5 mol of ethane, C2H6, undergo combustion according to the unbalanced equation C2H6+O2---->CO2+H2O, how many moles of oxygen are required? b. How many moles of each product are formed?

Expert's answer

If 4.5 mol of ethane, C_{2}H_{6}, undergo combustionaccording to the unbalanced equation the amount of O_{2} is the samethat amount of ethane.

C_{2}H_{6} + O_{2} ----> CO_{2} + H_{2}O, so it is 4.5 mol of O_{2}

But when it is balanced equation the amount of O_{2} is next,

C_{2}H_{6} + 7/2 O_{2} ----> 2CO_{2} + 3H_{2}O

4.5 mol* 7/2 = 15.72 mol

C

But when it is balanced equation the amount of O

C

4.5 mol* 7/2 = 15.72 mol

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