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प्रश्न
Calcium carbonate reacts with aqueous HCl to give CaCl2 and CO2 according to the reaction,
\[\ce{CaCO_{3(s)} + 2 HCl_{(aq)} → CaCl_{2(aq)} + CO_{2(g)} + H2O_{(l)}}\]
What mass of CaCO3 is required to react completely with 25 mL of 0.75 M HCl?
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उत्तर
0.75 M of HCl ≡ 0.75 mol of HCl are present in 1 L of water
≡ [(0.75 mol) × (36.5 g mol−1)] HCl is present in 1 L of water
≡ 27.375 g of HCl is present in 1 L of water
Thus, 1000 mL of solution contains 27.375 g of HCl.
∴ Amount of HCl present in 25 mL of solution
= `(27.375)/(1000) xx 25`
= 0.6844 g
From the given chemical equation,
\[\ce{CaCO_{3(s)} + 2 HCl_{(aq)} → CaCl_{2(aq)} + CO_{2(g)} + H2O_{(l)}}\]
2 mol of HCl (2 × 36.5 = 73 g) react with 1 mol of CaCO3 (100 g).
∴ Amount of CaCO3 that will react with 0.6844 g = `100/73 xx 0.6844`
= 0.9375 g
∴ The amount of CaCO3 that will react with 0.6844 g is 0.9375 g.
संबंधित प्रश्न
Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2) with aqueous hydrochloric acid according to the reaction
\[\ce{4HCl_{(aq)} + MnO_{2(s)} → 2H2O_{(l)} + MnCl_{2(aq)} + Cl_{2(g)}}\]
How many grams of HCl react with 5.0 g of manganese dioxide?
What mass of CaCl2 in grams would be enough to produce 14.35 gm of AgCl?
Production of iron in a blast furnace follows the following equation:
\[\ce{Fe3O4 (s) + 4CO (g) -> 3Fe (l) + 4CO2 (g)}\]
When 4.640 kg of Fe3O4 and 2.520 kg of CO are allowed to react then the amount of iron (in g) produced is:
[Given: Molar Atomic mass (g mol−1): Fe = 56
Molar Atomic mass (g mol−1): O = 16
Molar Atomic mass (g mol−1): C = 12]
