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Q. No.Which of the following statements is true regarding the reaction given below?
\(2 \mathrm{Al}_{(\mathrm{s})}+6 \mathrm{HCl}_{(\mathrm{aq})} \rightarrow 2 \mathrm{Al}^{3+}{ }_{(\mathrm{aq})}+6 \mathrm{Cl}^{-}_{(\mathrm{aq})}+3 \mathrm{H_2}_{\mathrm({g})}\)
| 1. | 6 L HCl(aq) is consumed for every 3L of H2(g) produced. |
| 2. | 33.6 L H2(g) is produced regardless of temperature and pressure for every mole of Al that reacts. |
| 3. | 67.2 L H2(g) at STP is produced for every mole of Al that reacts. |
| 4. | 11.2 L H2(g) at STP is produced for every mole of HCl(aq) consumed. |
Subtopic: Limiting Reagent |
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Level 3: 35%-60%
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250 mL of \(0.5~\text{M NaOH}\) was added to 500 mL of 1 M HCl. The number of unreacted HCl molecules in the solution after complete reaction is
\(x\times10^{21}.\) Find the value of x (Nearest integer).
\(\left(\mathrm{N}_{\mathrm{A}}=6.022 \times 10^{23}\right)\)
1. 256
2. 465
3. 226
4. 145
\(x\times10^{21}.\) Find the value of x (Nearest integer).
\(\left(\mathrm{N}_{\mathrm{A}}=6.022 \times 10^{23}\right)\)
1. 256
2. 465
3. 226
4. 145
Subtopic: Limiting Reagent |
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Level 2: 60%+
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When \(35 ~mL\) of \(0.15~ M\) lead nitrate solution is mixed with \(20 ~mL\) of \(0.12 ~M\) chromic sulphate solution, \(x× 10^{–5}\) moles of lead sulfate precipitate out. Calculate the value of \(x\). (Round off to the Nearest Integer)
| 1. | 525 | 2. | 124 |
| 3. | 734 | 4. | 223 |
Subtopic: Limiting Reagent |
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Level 3: 35%-60%
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When \(100 \mathrm{~g} ~\mathrm{CaCO}_3\) is reacted with \(\mathrm{0.19 ~mole}\) of \(\mathrm{HCl}\), the moles of \(\mathrm{CaCl}_2\) formed are \(\mathrm{\mathrm{P} \times 10^{-3} mol.}\) What is the value of \(\mathrm{P?}\)
1. 78
2. 95
3. 45
4. 63
1. 78
2. 95
3. 45
4. 63
Subtopic: Limiting Reagent |
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Level 2: 60%+
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Which of the following statements is incorrect if 14.0 gm of calcium metal is allowed to react with excess HCl at 1.0 atm pressure & 273 K?
[Molar mass in g/mol, Ca = 40, Cl = 35.5]
1. 0.35 mole of \(H_2\) gas is evolved
2. The limiting reagent is calcium metal
3. 33.3 g of \(CaCl_2\) is produced
4. 7.84 L of \(H_2\) gas is evolved
[Molar mass in g/mol, Ca = 40, Cl = 35.5]
1. 0.35 mole of \(H_2\) gas is evolved
2. The limiting reagent is calcium metal
3. 33.3 g of \(CaCl_2\) is produced
4. 7.84 L of \(H_2\) gas is evolved
Subtopic: Limiting Reagent | Equation Based Problem |
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Level 2: 60%+
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When 8.74 g MnO₂ is treated with HCl, what mass of Cl₂ (in grams) is liberated?
(Given: Molar mass of MnO₂ = 87.4 g/mol)
| 1. | 7.10 g | 2. | 17.1 g |
| 3. | 14.2 g | 4. | 3.55 g |
Subtopic: Limiting Reagent |
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Level 3: 35%-60%
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36 g of A react with 56 g of B to form \(AB_2\) according to given reaction :
\(A+2B\rightarrow AB_2\)
Which of the following is correct?
(Given : Molar mass of A = 60 g/mol, Molar mass of B = 80 g/mol)
1. Molecular weight of \(AB_2\) is 140.
2. A is limiting reagent.
3. 15 gm of A remains unreacted.
4. Weight of \(AB_2\) is 132 gm.
\(A+2B\rightarrow AB_2\)
Which of the following is correct?
(Given : Molar mass of A = 60 g/mol, Molar mass of B = 80 g/mol)
1. Molecular weight of \(AB_2\) is 140.
2. A is limiting reagent.
3. 15 gm of A remains unreacted.
4. Weight of \(AB_2\) is 132 gm.
Subtopic: Moles, Atoms & Electrons | Limiting Reagent | Equation Based Problem |
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