Ethyl Alcohol is oxidised on burning to Carbon dioxide and Water.

Calculate the no. of moles of oxygen required to produce 2.8 litres of Carbon dioxide at S.T.P.

 

Asked by malapandey8278 | 2nd Feb, 2019, 08:54: AM

Expert Answer:

1. 

Ethyl Alcohol is oxidised on burning to Carbon dioxide and Water.

 
Ethanol or ethyl alcohol is one of the hydrocarbon fuel used in laboratory and industries.
chemical formula:- CH3-CH2-OH or C2H5-OH. Like all hydro-carbon fuel, when ethanol is burnt in air,
it reacts with oxygen and the products of this reaction are CO2 and water. This reaction is an exothermic reaction and gives out a lot of heat energy.
 
C2H5-OH + 3O→ 2CO2 + 3H2O + energy
 
 
2. Calculate the no. of moles of oxygen required to produce 2.8 liters of Carbon dioxide at S.T.P.
 
    The reaction is,
 
    space straight C space space space space space plus space space straight O subscript 2 space space space space rightwards arrow space space space CO subscript 2 space
1 space mol space space space space space space 1 space mol space space space space space space space space 1 space mol

1 space mol space of space carbon space requires space 1 space mol space of space oxygen space to space form space 1 space mol space of space carbon space dioxide

1 space mol space of space straight O subscript 2 space gives space 22.4 space lit space of space CO subscript 2

2.8 space lit space of space CO subscript 2 space will space require comma space fraction numerator 2.8 over denominator 22.4 end fraction
space space
space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space space equals space 0.125 space mol space of space straight O subscript 2

Answered by Varsha | 4th Feb, 2019, 12:06: PM