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प्रश्न
112 cm3 of H2S(g) is mixed with 120 cm3 of Cl2(g) at STP to produce HCl(g) and sulphur(s). Write a balanced equation for this reaction and calculate
- the volume of gaseous product formed.
- composition of the resulting mixture.
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उत्तर
\[\ce{H2S + Cl2 -> 2HCl + S}\]
(i)
At STP,
1 mole gas occupies = 22.4 L.
1 mole H2S gas produces = 2 moles HCl gas,
∴ 22.4 L H2S gas produces
= 22.4 × 2
= 44.8 L HCl gas.
Hence, 112 cm3 H2S gas will produce
= 112 × 2
= 224 cm3 HCl gas.
Hence, 224 cm3 HCl gas is produced.
(ii)
1 mole H2S gas consumes = 1 mole Cl2 gas.
Hence, 22.4 L H2S gas consumes = 22.4 L Cl2 gas at STP.
∴ 112 cm3 H2S gas consumes = 112 cm3 Cl2 gas.
120 cm3 − 112 cm3 = 8 cm3 Cl2 gas remains unreacted.
Hence, the composition of the resulting mixture is 224 cm3 HCl gas + 8 cm3 Cl2 gas.
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?
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\[\ce{2C2H2_{(g)} + 5O2_{(g)}-> 4CO2_{(g)} + 2H2O_{(g)}}\]
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\[\ce{2NO + O2 → 2NO2}\]
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- 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.
