# 20 ml. each of oxygen and hydrogen and 10 ml. of carbon monoxide are exploded in an enclosure. What will be the volume and composition of the mixture of the gases when they are cooled to room temperature.

20 ml. each of oxygen and hydrogen and 10 ml. of carbon monoxide

[By Lussac’s law]

2CO     +     O2    →     3CO2

2 vol     :    1 vol  →     2 vol

To calculate the amount of CO2 produced,

CO     :     CO2

2        :     2

10      :     x

⇒ x = 2 × 10\over 2 = 10 ml

Therefore, CO2 produced is 10 ml

To calculate the amount of O2 used,

CO      :      O2

2 vol   :    1 vol

10 ml  :    x ml

⇒ x = 10 × 1\over 2 = 5 ml

From relation,

2H2      +      O2      →     2 H2O

2 vol     :     1 vol     →     2 vol

To calculate the amount of O2 used,

H       :      O2

2 vol    :    1 vol

20 ml  :    x ml

⇒ x = 20 × 1\over 2 = 10 ml

Therefore, total vol. of oxygen used = 10 + 5 = 15 ml

Hence, oxygen left = 20 – 15 = 5 ml

Therefore, oxygen left is 5 ml and CO2 produced is 10 ml.

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