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Under the same pressure and temperature,...

Under the same pressure and temperature, a mixture of 100 mL of water gas and 100 mL of `O_(2)` is subjected to explosion. Find the composition of the gas mixture formed by explosion under the same conditions of pressure and temperature.

Text Solution

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Water gas is an equimolecular mixture of CO and `H_(2)` (mixture of same volume of CO and `H_(2)`).
So, 100 mL of water gas contains 50 mL each of CO and `H_(2)`.
The reactions caused by explosion are:
`2CO+O_(2) to 2CO_(2)` . . .[1]
`2H_(2)+O_(2) to 2H_(2)O` . .. .[2]
From equation [1], it is seen that under the same conditions of temperature and pressure, 1 volume of `O_(2)` reacts with 2 vols. of CO to form of `CO_(2)`.
so, under same conditions of temperature and pressure, volume of `O_(2)` required for 50 mL of CO=25 mL. and volume of `CO_(2)` formed=50 mL.
According to equation [2], under the same conditions of temperature and pressure, volume of `O_(2)` required to react with 50 mL of `H_(2)=25 mL` and volume of water vapour, produced by the reaction=50 mL.
`therefore`Total volume of `O_(2)` used up in the two reactions
=(25+25)=50 mL.
Hence after explosion, both the volumes of `CO_(2)` and `H_(2)O` produced is 50 mL while the volume of unreacted `O_(2)`
=(100-50)=50 mL.
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