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
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.
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?
What volume of oxygen would be required to burn completely 400 ml of acetylene [C2H2]? Also calculate the volume of carbon dioxide formed.
\[\ce{2C2H2 + 5H2O -> 4CO2 + 2H2O(l)}\]
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.
Ammonia may be oxidised to nitrogen monoxide in the presence of a catalyst according to the following equation.
\[\ce{4NH3 + 5O2 → 4NO + 6H2O}\]
If 27 litres of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?
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.
The volumes of gases A, B, C and D are in the ratio, 1 : 2 : 2 : 4 under the same conditions of temperature and pressure.
- Which sample of gas contains the maximum number of molecules?
- If the temperature and pressure of gas A are kept constant, then what will happen to the volume of A when the number of molecules is doubled?
- If this ratio of gas volume refers to the reactants and products of a reaction, which gas law is being observed?
- If the volume of A is actually 5.6 dm3 at STP, calculate the number of molecules in the actual Volume of D at STP (Avogadro's number is 6 × 1023).
- Using your answer from (iv), state the mass of D if the gas is dinitrogen oxide (N2O).
