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Q. No.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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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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For the reaction:
\(Cl_2 + KOH \rightarrow KCl + KClO + H_2O\)
1 mole of \(Cl_2\) passed into 2 litre, 2M solution of KOH. Determine the molarity of \(Cl^-, ClO^-\) and \(OH^-\) respectively.
1. 1 M, 0.5 M, 0.5 M
2. 0.5 M, 0.5 M, 1 M
3. 1 M, 1 M, 0.5 M
4. 0.5 M, 1 M, 0.5 M
\(Cl_2 + KOH \rightarrow KCl + KClO + H_2O\)
1 mole of \(Cl_2\) passed into 2 litre, 2M solution of KOH. Determine the molarity of \(Cl^-, ClO^-\) and \(OH^-\) respectively.
1. 1 M, 0.5 M, 0.5 M
2. 0.5 M, 0.5 M, 1 M
3. 1 M, 1 M, 0.5 M
4. 0.5 M, 1 M, 0.5 M
Subtopic: Moles, Atoms & Electrons | Concentration Based Problem | Equation Based Problem |
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100 g of 98% by weight \(H_2SO_4\) is mixed with 100 gm of 49% by weight \(H_2SO_4 .\) Determine the mole fraction of \(H_2SO_4\) in the final solution:
1. 0.9
2. 0.1
3. 0.67
4. 0.33
1. 0.9
2. 0.1
3. 0.67
4. 0.33
Subtopic: Moles, Atoms & Electrons | Concentration Based Problem |
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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 |
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For Balanced chemical reaction:
Which of the following is correct?
| \(2 \mathrm{Al}_{(\mathrm{s})}+6 \mathrm{HCl}_{\mathrm{aq}} \rightarrow 2 \mathrm{AlCl}_3+3 \mathrm{H}_{2(\mathrm{~g})}\) |
Which of the following is correct?
| 1. | With excess of Al, volume of \(H_2\) gas produced per mole of HCl reacted will be 33.6 L at 1 atm & 273 K. |
| 2. | With excess of Al, volume of \(H_2\) gas produced per mole of HCl reacted will be 11.2 L at 1 atm & 273 K. |
| 3. | With excess of HCI, moles of \(AlCl_3\) produced per mole of AI reacted are 2. |
| 4. | At given P and T, 12 L HCI produced 6 L \(H_2 \) gas. |
Subtopic: Moles, Atoms & Electrons | Concentration Based Problem |
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2.8 × 10–3 mol of CO2 is left after removing 1021 molecules from its ‘x’ mg sample. The mass of CO2 taken initially is:
(Given : \(\mathrm{N}_{\mathrm{A}}=6.02 \times 10^{23} \mathrm{~mol}^{-1}\))
(Given : \(\mathrm{N}_{\mathrm{A}}=6.02 \times 10^{23} \mathrm{~mol}^{-1}\))
| 1. | 196.2 mg | 2. | 98.3 mg |
| 3. | 150.4 mg | 4. | 48.2 mg |
Subtopic: Moles, Atoms & Electrons |
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Concentrated nitric acid is labelled as 75% by mass. The volume in mL of the solution which contains 30 g of nitric acid is:
Given: The density of nitric acid solution is 1.25 g/mL
1. 45
2. 55
3. 32
4. 40
Given: The density of nitric acid solution is 1.25 g/mL
1. 45
2. 55
3. 32
4. 40
Subtopic: Millimole/Equivalent Concept |
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Which of the following mixtures of 1M base and 1M acid leads to the largest increase in temperature?
1. 30 mL HCl and 30 mL NaOH
2. 30 mL CH3COOH and 30 mL NaOH
3. 50 mL HCl and 20 mL NaOH
4. 45 mL CH3COOH and 25 mL NaOH
1. 30 mL HCl and 30 mL NaOH
2. 30 mL CH3COOH and 30 mL NaOH
3. 50 mL HCl and 20 mL NaOH
4. 45 mL CH3COOH and 25 mL NaOH
Subtopic: Moles, Atoms & Electrons | Concentration Based Problem | Millimole/Equivalent Concept |
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A compound consists of 54.2% carbon (C), 9.2% hydrogen (H), and 36.6% oxygen (O) by mass. The molar mass of the compound is 132 g/mol.
Determine the molecular formula of the compound.
(Given -Relative atomic masses: C = 12, H = 1, O = 16)
| 1. | \(\mathrm{C}_4 \mathrm{H}_9 \mathrm{O}_3\) | 2. | \(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6\) |
| 3. | \(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_3\) | 4. | \(\mathrm{C}_4 \mathrm{H}_8 \mathrm{O}_2\) |
Subtopic: Empirical & Molecular Formula |
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