Question

3. 200 cm^3 of methane at 27°C and 760 mm pressure of Hg were exploded with excess of oxygen
Determine the volume of CO2 at NT.P.
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Answer 1

Answer:

179.2cm^3

Explanation:

CH4+ 02 ---> CO2+ H20

On balancing,

CH4 + 2 02. ----> CO2 + 2H20

Converting values,

200cm^3= 200ml= 0.2L

27°C= 300K

760mmHg= 1 atm

Using Ideal Gas Equation,

PV=nRT

n= PV/RT

n= 1*0.2/(1/12)*300

n= 0.2/25

n=0.008 moles of methane

Therefore,

Moles of CO2 produced= 1*(0.008)

=0.008 moles

Therefore volume produced,

0.008*22.4L = 0.1792L

Or

179.2mL or 179.2 cm^3