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प्रश्न
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.
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उत्तर १
- 6 litres of hydrogen and 4 litres of chlorine when mixed, results in the formation of 8 litres ofHCl gas.
- When water is added to it, it results in the formation of hydrochloric acid. Chlorine acts as a limiting agent leving behind only 2 litres of hydrogen gas.
iii. Therefore, the volume of the residual gas will be 2 litres.
उत्तर २
\[\ce{H2 + Cl2 -> 2HCl}\]
1 vol. 1 vol. 2 vol.
1 lit. 1 lit. 2 lit.
1 lit. of H2 can use 1 lit. of Cl2
∴ 4 lit. of H2 can be combined with 4 lit. of Cl2
\[\ce{H2 + Cl2 -> 2HCl}\]
6 lit. 4 lit.
1 lit of H2 + 1 lit of Cl2 = 2 lit of HCl
4 lit of H2 forms 2 x 4 = 8 lit HCl
Hence after reaction 8 lit of HCl + 2 lit of H2 i.e. 10 lit
When water is added to the gases formed HCl dissolves and residual gas is 2 lit. H2·
संबंधित प्रश्न
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?
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.
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)
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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?
A mixture of hydrogen and chlorine occupying 36 cm3 was exploded. On shaking it with water, 4 cm3 of hydrogen was left behind. Find the composition of the mixture.
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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\[\ce{2C2H2_{(g)} + 5O2_{(g)} → 4CO2_{(g)} + 2H2O_{(g)}}\]
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).
