Advertisements
Advertisements
Question
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?
Advertisements
Solution
Given:
C3H8 + 5O2 → 3CO2 + 4H2O
Volume of air = 1000 cm3
Percentage of oxygen in air = 20%
From the given information
C3H8 + 5O2 → 3CO2 + 4H2O
1vol 5vols 3vols 4vols
According to Gay-Lussac’s law,
1 vol. of propane consumes 5 vol. of oxygen
Volume of oxygen = 1000 cm3 × 20% = 200 cm3
Therefore,
Volume of propane burnt for every 200 cm3 of oxygen
`= 1/5 xx 200 = 40 cm^3`
40 cm3 of propane is burnt.
APPEARS IN
RELATED QUESTIONS
State Gay-Lussac’s law of combining volumes.
When gases react their volumes bear a simple ratio to each other, under the same conditions of temperature and pressure. Who proposed this gas law?
What volume of oxygen would be required for complete combustion of 100L of ethane according to the following equation?
2C2H6 + 7O2 → 4CO2 + 6H2O
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.
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.
\[\ce{2C2H2_{(g)} + 5O2_{(g)}-> 4CO2_{(g)} + 2H2O_{(g)}}\]
450 cm3 of nitrogen monoxide and 200 cm3 of oxygen are mixed together and ignited. Caclulate the composition of resulting mixture.
\[\ce{2NO + O2 → 2NO2}\]
What volume of air (containing 20% O2 by volume) will be required to burn completely 10 cm3 of methane and acetylene?
\[\ce{CH4 + 2O2 → CO2 + 2H2O}\]
\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]
LPG has 60% propane and 40% butane: 10 litres of this mixture is burnt. Calculate the volume of carbon dioxide added to atmosphere.
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
\[\ce{2C4H10 + 13O2 → 8CO2 + 10H2O}\]
1250 cc of oxygen was burnt with 300cc of ethane [C2H6]. Calculate the volume of unused oxygen formed:
\[\ce{2C2H6 + 7O2 -> 4CO2 + 6H2O}\]
Which amongst the following options is the correct graphical representation of Boyle’s law?
