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A 1 L sample of CH4 and O2 measured at 2...

A 1 L sample of `CH_4 and O_2` measured at `25^@C` and 740 torr were allowed to react at constant pressure in calorimeter which together with its contents had a heat capacity of 1260 cals/K. The complete combustion of `CH_4` to `CO_2` and `H_2O` caused a temperature rise in calorimeter 0.667 K. What was the mole per cent of `CH_4` in the original mixture? `(DeltaH)` combustion of `CH_4(g) = – 210.8 kcals//"mole"`.

Text Solution

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Applying PV = nRT for gaseous mixture.
`(740/760) xx 1 xx 0.082 xx 298`
`n=0.0398`
Heat generated = Heat capacity `xx` Temperature rise
`=1260 xx 0.667 = 840 cal`
Mole of `CH_(4)` in the mixture `=840/(210.8 xx 10^(3)) = 3.98 xx 10^(-3)`
Mole per cent of `CH_(4)= (3.98 xx 10^(-3))/0.398 xx 100 =10`
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