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Q. No.A solution contains 25% water, 25% ethanol \((C_2H_5OH)\) and 50% acetic acid \((CH_3COOH)\) by mass. The mole fraction of:
(a) Water \(=0.502\)
(b) Ethanol \(=0.302\)
(c) Acetic acid \(=0.196\)
(d) Ethanol + Acid \(=0.497\)
Choose the correct option:
1. (a), (b)
2. (c), (d)
3. (a), (d)
4. None of the above
(a) Water \(=0.502\)
(b) Ethanol \(=0.302\)
(c) Acetic acid \(=0.196\)
(d) Ethanol + Acid \(=0.497\)
Choose the correct option:
1. (a), (b)
2. (c), (d)
3. (a), (d)
4. None of the above
Subtopic: Concentration Based Problem |
55%
Level 3: 35%-60%
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1 gram of sodium hydroxide was treated with 25 mL of 0.75 M HCl solution, the mass of sodium hydroxide left unreacted is equal to :
1. 250 mg
2. Zero mg
3. 200 mg
4. 750 mg
1. 250 mg
2. Zero mg
3. 200 mg
4. 750 mg
Subtopic: Millimole/Equivalent Concept |
54%
Level 3: 35%-60%
NEET - 2024
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NEET 2026 - Target Batch - Vital
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NEET 2026 - Target Batch - Vital
Consider the given two statements:
Select the correct option:
| Statement I: | The law of multiple proportions is followed by the gases SO2 and SO3, but not by CO and CO2. |
| Statement II: | Dalton’s theory explains the laws of chemical combination as well as laws of gaseous volumes. |
| 1. | Statement I is correct, and Statement II is correct. |
| 2. | Statement I is incorrect, and Statement II is correct. |
| 3. | Statement I is correct, and Statement II is incorrect. |
| 4. | Statement I is incorrect, and Statement II is incorrect. |
Subtopic: Introduction |
53%
Level 3: 35%-60%
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| Assertion (A): | Irrespective of the source, a given compound always contains the same elements in the same proportion. |
| Reason (R): | This law is referred to as the law of multiple proportions. |
| 1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |
| 3. | (A) is true but (R) is false. |
| 4. | Both (A) and (R) are false. |
Subtopic: Introduction |
52%
Level 3: 35%-60%
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The number of moles of hydrogen gas liberated when 39 g of potassium reacts with 7.8 g of water is:
1. 0.22 mol
2. 0.43 mol
3. 0.50 mol
4. 1.0 mol
1. 0.22 mol
2. 0.43 mol
3. 0.50 mol
4. 1.0 mol
Subtopic: Equation Based Problem |
Level 3: 35%-60%
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What is the concentration of nitrate ions in 40.0 mL of a 0.25 M solution of copper(II) nitrate?
1. 0.010 M
2. 0.020 M
3. 0.050 M
4. 0.50 M
1. 0.010 M
2. 0.020 M
3. 0.050 M
4. 0.50 M
Subtopic: Concentration Based Problem |
Level 3: 35%-60%
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What will be the mass of one atom of \(^{12}C\)?
1. 1 a.m.u.
2. \(1.9923\times10^{-23}~\text{g}\)
3. \(1.6603\times10^{-22}~\text{g}\)
4. 6 a.m.u.
Subtopic: Moles, Atoms & Electrons | Introduction |
Level 3: 35%-60%
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Consider the given two statements:
In the light of above statements, choose the correct option from the following :
| Statement I: | 1 amu is defined as the mass exactly equal to one-twelfth of the mass of one carbon-12 atom. |
| Statement II: | Number of atoms in 8 u of He is 2NA. |
| 1. | Both Statement I and Statement II are correct. |
| 2. | Both Statement I and Statement II are incorrect. |
| 3. | Statement I is correct but Statement II is incorrect. |
| 4. | Statement I is incorrect but Statement II is correct |
Subtopic: Introduction |
Level 3: 35%-60%
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A 1.00 g sample of which compound will produce the greatest amount of carbon dioxide after complete combustion with excess oxygen?
1. CH4
2. C3H8
3. C6H6
4. C8H18
1. CH4
2. C3H8
3. C6H6
4. C8H18
Subtopic: Equation Based Problem |
Level 3: 35%-60%
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Which of the following has the maximum mass?
1. 0.1 gram molecule of oxygen.
2. 10 ml \(H_2O \) at STP
3. \(3.01 \times 10^{22}\) molecules of \(H_2SO_4\)
4. 1 gram atom of hydrogen.
1. 0.1 gram molecule of oxygen.
2. 10 ml \(H_2O \) at STP
3. \(3.01 \times 10^{22}\) molecules of \(H_2SO_4\)
4. 1 gram atom of hydrogen.
Subtopic: Moles, Atoms & Electrons |
Level 4: Below 35%
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