Advertisements
Advertisements
प्रश्न
What volume of air (containing 20% O2 by volume) will be required to burn completely 10 cm3 of methane and acetylene?
\[\ce{CH4 + 2O2 → CO2 + 2H2O}\]
\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]
Advertisements
उत्तर
Methane + Oxygen
\[\ce{\underset{10 cm^3}{\underset{1 V}{CH4} + \underset{2 V}{2O2}} -> CO2 + 2H2O}\]
∴ Volume of \[\ce{O2}\] required = 10 × 2 = 20 cm3
∴ Volume of air = 20 × 5 = 100 cm3
∴ 20 cc of \[\ce{O2}\] is contained in 100 cm3 of air.
Acetylene + Oxygen
\[\ce{\underset{10 cm^3}{\underset{2 V}{2C2H2} + \underset{5 V}{5O2}} -> 4CO2 + 2H2O}\]
∴ Volume of \[\ce{O2}\] required = `5/2 xx 10 = 25` cm3
Total O2 needed = 20 + 25
= 45 cm3
Air conrains 20% oxygen,
∴ Air volume = `45/0.20`
= 225 cm3
APPEARS IN
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?
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.
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.
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).
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.
112 cm3 of H2S(g) is mixed with 120 cm3 of Cl2(g) at STP to produce HCl(g) and sulphur(s). Calculate composition of the resulting mixture.
