- 1(current)
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 |
52%
Level 3: 35%-60%
Please attempt this question first.
Hints
Please attempt this question first.
Consider the above reaction, the limiting reagent of the reaction and number of moles of NH3 formed respectively are:
1. \(\mathrm{H}_2, 1.42 \text { moles }\)
2. \(\mathrm{H}_2, 0.71 \text { moles }\)
3. \(\mathrm{N}_2, 1.42 \text { moles }\)
4. \(\mathrm{N}_2, 0.71 \text { moles }\)
Subtopic: Limiting Reagent |
75%
Level 2: 60%+
Please attempt this question first.
Hints
Please attempt this question first.
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 |
72%
Level 2: 60%+
Please attempt this question first.
Hints
Please attempt this question first.
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 |
55%
Level 3: 35%-60%
Please attempt this question first.
Hints
Please attempt this question first.
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 |
71%
Level 2: 60%+
Please attempt this question first.
Hints
Please attempt this question first.
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 |
73%
Level 2: 60%+
Please attempt this question first.
Hints
Please attempt this question first.
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 |
60%
Level 2: 60%+
Please attempt this question first.
Hints
Please attempt this question first.
36 g of A reacts with 56 g of B to form AB₂ according to the following reaction:
A + 2B → AB₂ . Which of the following statements is correct?
(Given: Molar mass of A = 60 g mol⁻¹ and molar mass of B = 80 g mol⁻¹)1. The molecular mass of AB₂ is 140 g mol⁻¹.
2. A is the limiting reagent.
3. 15 gm of A remains unreacted.
4. The mass of AB₂ formed is 132 g.
Subtopic: Moles, Atoms & Electrons | Limiting Reagent | Equation Based Problem |
68%
Level 2: 60%+
Please attempt this question first.
Hints
Please attempt this question first.
- 1(current)
Q. No.
© 2026 GoodEd Technologies Pvt. Ltd.