Advertisements
Advertisements
प्रश्न
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.
Advertisements
उत्तर
This experiment supports Gay Lussac’s law of combining volumes.
According to Gay lussac’s law, the volumes of gases reacting should be in a simple ratio.
\[\ce{CH4 + 2O2 → CO2 + 2H2O}\]
1V 2V 1V 0V
24 cc 48 cc 24 cc
1 vol. of CH4 requires O2 = 2 vols.
∴ 24 cc of CH4 requires O2 = 2 × 24 = 48 cc
Similarly, 24 cc of CH4 produce CO2 = 24 cc
∴ Vol. of O2 unused = 106 − 48 = 58cc
∴ Vol. of mixture on cooling = unused oxygen + CO2 formed
= 58 + 24
= 82 cc
APPEARS IN
संबंधित प्रश्न
State Gay-Lussac’s law of combining volumes.
How does Avogadro's law explain Gay - lussac's law of combining volumes?
What volume of oxygen would be required for complete combustion of 100L of ethane according to the following equation?
2C2H6 + 7O2 → 4CO2 + 6H2O
Calcium carbide is used for the artificial ripening of fruits. Actually the fruit ripens because of the heat evolved while calcium carbide reacts with the moisture. During this reaction calcium hydroxide and acetylene gas are formed. If 200 cm3 of acetylene is formed from a certain mass of calcium carbide, find the volume of oxygen required and carbon dioxide formed during the complete combustion. The combustion reaction can be represented as below.
\[\ce{2C2H2_{(g)} + 5O2_{(g)}-> 4CO2_{(g)} + 2H2O_{(g)}}\]
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?
450 cm3 of nitrogen monoxide and 200 cm3 of oxygen are mixed together and ignited. Caclulate the composition of resulting mixture.
\[\ce{2NO + O2 → 2NO2}\]
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.
200 cm3 of CO2 is collected at STP when a mixture of acetylene and oxygen is ignited. Calculate the volume of acetylene and oxygen at STP. in original mixture.
\[\ce{2C2H2_{(g)} + 5O2_{(g)} → 4CO2_{(g)} + 2H2O_{(g)}}\]
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.
Which amongst the following options is the correct graphical representation of Boyle’s law?
