Q. No.A 14.0 g sample of calcium metal reacts completely with excess hydrochloric acid (HCl) at 273 K and 1 atm pressure.
Which of the following statements regarding the reaction is incorrect?
Given: Molar masses: Ca = 40 g mol⁻¹, Cl = 35.5 g mol⁻¹
1. 0.35 mol of H₂ gas is evolved.
2. Calcium acts as the limiting reagent.
3. 33.3 g of CaCl₂ is formed.
4. 7.84 L of H₂ gas is evolved.
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 |
\(Cl_2 + KOH \rightarrow KCl + KClO + H_2O\)
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
Find the mole fraction of H₂SO₄ in the final solution.
1. 0.9
2. 0.1
3. 0.67
4. 0.33
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.
| \(2 \mathrm{Al}_{(\mathrm{s})}+6 \mathrm{HCl}_{\mathrm{aq}} \rightarrow 2 \mathrm{AlCl}_3+3 \mathrm{H}_{2(\mathrm{~g})}\) |
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. |
(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 |
Given: The density of nitric acid solution is 1.25 g/mL
1. 45
2. 55
3. 32
4. 40
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
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. | \(\mathrm{C}_4 \mathrm{H}_8 \mathrm{O}_2\) |
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