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Q. No.Dalton's Atomic theory could not explain which of the following?
1. Law of multiple proportion
2. Law of gaseous volume
3. Law of conservation of mass
4. Law of constant proportion
1. Law of multiple proportion
2. Law of gaseous volume
3. Law of conservation of mass
4. Law of constant proportion
Subtopic: Introduction |
68%
Level 2: 60%+
NEET - 2025
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Select the correct statements from the following:
Choose the correct answer from the options given below:
| A: | Atoms of all elements are composed of two fundamental particles. |
| B: | The mass of the electron is \(9.10939 \times 10^{-31} \mathrm{~kg} \text {. }\) |
| C: | All the isotopes of a given element show the same chemical properties. |
| D: | Protons and electrons are collectively known as nucleons. |
| E: | Dalton's atomic theory regarded the atom as an ultimate particle of matter. |
| 1. | B, C and E only | 2. | A, B and C only |
| 3. | C, D and E only | 4. | A and E only |
Subtopic: Introduction |
76%
Level 2: 60%+
NEET - 2023
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Consider the following data of compounds:
Which of the following represents a correct set of compounds having an equal number of atoms?
1. B, C, and D only
2. B, D, and E only
3. A, B, and C only
4. A, B, and D only
| A. | \(212 ~g ~\text{of}~Na_2CO_3 (s) \text{[molar mass}=106 ~g]\) |
| B. | \(~248 g ~\text{of}~ {Na}_2 \mathrm{O}({s}) [\text{molar mass} =62 \mathrm{~g} ]\) |
| C. | \(240 g ~\text{of} ~NaOH (s)~ [\text{molar mass} =40 \mathrm{~g} \) |
| D. | \( 12 g~ \text{of}~ \mathrm{H}_2(\mathrm{~g})[ \text{molar mass} =2 \mathrm{~g}].\) |
| E. | \( 220 g~ \text{of} ~\mathrm{CO}_2(\mathrm{~g})[\text{ molar mass }=44 \mathrm{~g}]\) |
1. B, C, and D only
2. B, D, and E only
3. A, B, and C only
4. A, B, and D only
Subtopic: Moles, Atoms & Electrons |
58%
Level 3: 35%-60%
NEET - 2025
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Match List-I with List-II:
| List-I (Quantities) |
List-II (Corresponding Values) |
||
| (a) | 4.48 litres of O2 at STP | (i) | 0.2 mole |
| (b) | 12.022 × 1022 molecules of H2O | (ii) | 12.044 × 1023 molecules |
| (c) | 96 g of O2 | (iii) | 6.4 g |
| (d) | 88 g of CO2 | (iv) | 67.2 litres at STP |
Choose the correct answer from the options given below:
| (a) | (b) | (c) | (d) | |
| 1. | (i) | (iii) | (iv) | (ii) |
| 2. | (iii) | (i) | (iv) | (ii) |
| 3. | (iv) | (i) | (ii) | (iii) |
| 4. | (iii) | (i) | (ii) | (iv) |
Subtopic: Moles, Atoms & Electrons |
50%
Level 3: 35%-60%
NEET - 2022
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Which of the following contains the maximum number of atoms ?
| 1. | 1 g of Mg(s) | 2. | 1 g of O2 (g) |
| 3. | 1 g of Li(s) | 4. | 1 g of Ag(s) |
Subtopic: Moles, Atoms & Electrons |
79%
Level 2: 60%+
NEET - 2020
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The maximum number of water molecules among the following is:
1. 18 mL of water
2. 0.18 g of water
3. 0.00224 L water vapours at 1 atm and 273 K
4. 10-3 mol of water
1. 18 mL of water
2. 0.18 g of water
3. 0.00224 L water vapours at 1 atm and 273 K
4. 10-3 mol of water
Subtopic: Moles, Atoms & Electrons |
59%
Level 3: 35%-60%
NEET - 2018
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Links
If Avogadro number \(N_{A}\), is changed from \(6 . 022 \times \left(10\right)^{23}\)\(\text{mol}^{- 1}\) to \(6 . 022 \times \left(10\right)^{20} ~\text{mol}^{- 1}\) this would change the:
| 1. | Definition of mass in units of grams |
| 2. | Mass of one mole of carbon |
| 3. | Coefficient of chemical species in a balanced equation |
| 4. | Ratio of elements in a compound |
Subtopic: Moles, Atoms & Electrons |
73%
Level 2: 60%+
NEET - 2015
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When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), both at STP, the moles of HCl(g) formed are equal to:
1. 1 mol of HCl(g)
2. 2 mol of HCl(g)
3. 0.5 mol of HCl(g)
4. 1.5 mol of HCl(g)
Subtopic: Moles, Atoms & Electrons |
72%
Level 2: 60%+
AIPMT - 2014
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4.74 g of an inorganic compound contains 0.39g of K, 0.27 g of Al, 1.92 g of \(\mathrm{SO_4}\) radicals and 2.16 g of water. If molar mass of the compound is \(948 \mathrm{~g} \mathrm{~mol}^{-1},\) the molecular formula of the inorganic compound is:
| 1. | \(\mathrm{{KAl}({SO}_4)_2 \cdot 12 {H}_2 {O}}\) |
| 2. | \(\mathrm{{K}_2 {Al}_2({SO}_4)_6 \cdot 12 {H}_2 {O}}\) |
| 3. | \(\mathrm{{K}_2 {SO}_4 \cdot {Al}_2({SO}_4)_3 \cdot24 {H}_2 {O}}\) |
| 4. | \(\mathrm{{K}_2 {SO}_6 \cdot {Al}_2({SO}_4)_3 \cdot12 {H}_2 {O}}\) |
Subtopic: Empirical & Molecular Formula |
59%
Level 3: 35%-60%
NEET - 2024
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A compound X contains 32% of A, 20% of B and remaining percentage of C. Then, the empirical formula of X is :
(Given atomic mass of A = 64; B = 40; C = 32u)
1. ABC3
2. AB2C2
3. ABC4
4. A2BC2
(Given atomic mass of A = 64; B = 40; C = 32u)
1. ABC3
2. AB2C2
3. ABC4
4. A2BC2
Subtopic: Empirical & Molecular Formula |
77%
Level 2: 60%+
NEET - 2024
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