2. A sample of coal gas contained 45% H2, 30% CH4, 20% CO and 5% CH2 by volume. 100 cm?
of this gaseous mixture was mixed with 190 cm of oxygen and exploded. Calculate the volume
and composition of the mixture, when cooled to room temperature and pressure.
answer -(85 cm residual oxygen, 60cmº CO2 and 145 cm3 total volume)
Answers
Answer:
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Explanation:
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Given :
According to the question;
100 mL of gasoeus mixture will contain:
45mL of hygrogen
30 mL of Methane
20 mL of carbon monoxide
5 mL of Ethyne
Explanation:
Equations representing the following combustion : (In the question it is given as mixture is mixed with oxygen therefore all constituents should react with oxygen)
(i) Hygrogen
2H2 + O2 --> 2H2O
2 vol 1vol Nil
2 vol of hydrogen requires 1 vol of oxygen
Therefore, 1 vol of hydrogen requires 1/2 vol of oxygen
=> 45 mL of oxygen requires 1/2*45 mL of oxygen
= 22.5mL of oxygen
(ii) Methane
CH4 + 2O2 --> CO2 + 2H2O
1 vol 2vol 1 vol nil
* 1 vol of CH4 requires 2 vol of O2
Therefore, 30 mL of methane requires 30*2 mL of oxygen
= 60 mL of oxygen
* 1 vol of methane produces 1 vol of CO2
Therefore, 30mL of methane produces 30 mL of CO2
=30 mL of CO2
Do all other constituents in same manner and last add all the oxygen used up = 105 mL and all the carbon dioxide formed = 60mL
Volume of oxygen used up = (total volume - vol of oxygen used)
= 55 mL
Total carbon dioxide formed = 60mL
Therefore, Total volume of gases left = 55+60=115 mL
Answer :
55 mL residual oxygen and 60 mL carbon dioxide and 115 mL total volume.