# 2C2H6 + 7O2 → 4CO2 + 6H2O l C2H6 5) How many liters of Carbon Dioxide would be produced if 16.00 L of ethane, (C2H6), were burnt (all at STP)? At STP volume of an ideal gas is 22.4L/mol.

Therefore;

Volume of ethane mixed = `16L`

Amount of Ethane mixed = `16/22.4`

Mole ratio

`C_2H_6:CO_2 = 2:4 = 1:2`

Amount of `CO_2` produced = `(16/22.4)*2`

Volume of `CO_2` produced = `(16/22.4)*2*22.4 = 32 L`

So there will be 32L of `CO_2` will be produced.

assumptions

`CO_2` and `C_2H_6` act as ideal gasses at the given conditions.

Approved by eNotes Editorial Team Balanced chemical equation:

2C2H6 + 7O2  --> 4 CO2 + 6H2O

Using stoichiometry,

2 moles of ethane produce 4 moles of CO2.

Given volume of ethane gas = 16 lt.

At STP, 1 mole of a gas = 22.4 lt of gas

In the present case, 2 moles of ethane = 2x22.4 = 44.8 lts of ethane produces 4 x 22.4 lts (= 89.6 lts) of CO2

therefore, using unitary method,

16 l of ethane will produce = 89.6 x 16/44.8 lts of CO2 = 32 lts of CO2.

Approved by eNotes Editorial Team