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प्रश्न
LPG has 60% propane and 40% butane: 10 litres of this mixture is burnt. Calculate the volume of carbon dioxide added to atmosphere.
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
\[\ce{2C4H10 + 13O2 → 8CO2 + 10H2O}\]
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उत्तर
Ratio of propane and Butane in mixture
= 60 : 40
= 3 : 2
Ratio in 10 litres mixture = `3/5 xx 10 and 2/5 xx 10`
= 6 lit : 4 lit
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
1 vol 3 vol
1 volume of propane produces CO2 = 3 volumes
∴ 6 litres produces CO2 = 3 x 6
= 18 litres ...(i)
\[\ce{2C4H10 + 13O2 → 8CO2 + 10H2O}\]
2 vol 8 vol
2 litres of Butane produces CO2 = 8 litres
∴ 4 litres produce CO2 = `(8 xx 4)/2`
= 16 litres ...(ii)
∴ CO2 added to atmosphere = 18 + 16
= 34 litres.
संबंधित प्रश्न
Propane burns in air according to the following equation:
C3H8 + 5O2 → 3CO2 + 4H2O
What volume of propane is consumed on using 1000 cm3 of air, considering only 20% of air contains oxygen?
State Gay-Lussac's law of combining volumes.
The reaction 4N2O + CH4 → CO2 + 2H2O + 4N2 takes place in the gaseous state. If the volumes of all the gases are measured at the same temperature, and pressure, calculate the volume of dinitrogen oxide (N2O), required to give 150cm3 of steam.
Propane burns in air according to the following equation:
\[\ce{C3H8 + 5O2 -> 3CO2 + 4H2O}\]
What volume of propane is consumed on using 1000 cm3 of air, considering only 20% of air contains oxygen?
24 cc Marsh gas (CH4) was mixed with 106 cc oxygen and then exploded. On cooling the volume of the mixture became 82 cc, of which, 58 cc was unchanged oxygen. Which law does this experiment support? Explain with calculations.
1250 cc of oxygen was burnt with 300cc of ethane [C2H6]. Calculate the volume of carbon dioxide formed:
\[\ce{2C2H6 + 7O2 -> 4CO2 + 6H2O}\]
What volume of propane is burnt for every 500 cm3 of air used in the reaction under the same conditions? (assuming oxygen is `1/5`th of air)
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
If 6 liters of hydrogen and 4 liters of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas.
The reaction: \[\ce{4N2O + CH4 -> CO2 + 2H2O + 4N2}\] takes place in the gaseous state. If all volumes are measured at the same temperature and pressure, calculate the volume of dinitrogen oxide (N2O) required to give 150 cm3 of steam.
112 cm3 of H2S(g) is mixed with 120 cm3 of Cl2(g) at STP to produce HCl(g) and sulphur(s). Calculate the volume of gaseous product formed.
