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Q. No.Consider the two statements:
Statement I:
Scientific notation for 0.00016 is \(1.6 \times 10^{-3} \).
Statement II:
The volume of water to be added to change the molarity of 200 mL
0.5 M aqueous solution to 0.1 M is 800 mL
1.
Statement I is correct, Statement II is correct.
2.
Statement I is incorrect, Statement II is correct.
3.
Statement I is correct, Statement II is incorrect.
4.
Statement I is incorrect, Statement II is incorrect.
0.5 M aqueous solution to 0.1 M is 800 mL
Subtopic: Introduction |
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How many chlorine atoms are in 1.00 mL of CCl4 (M=153.8, density=1.59 g mL-1)?
1. 1.56×1021
2. 6.23×1021
3. 1.57×1022
4. 2.49×1022
1. 1.56×1021
2. 6.23×1021
3. 1.57×1022
4. 2.49×1022
Subtopic: Moles, Atoms & Electrons |
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In the following reaction:
\(4HCl + MnO_2 \rightarrow 2H_2O + MnCl_2 + Cl_2\)
Amount(in g) of manganese dioxide that reacts with 7.3 g of HCl is:
(Atomic weight of Mn is 55)
1. 0.23
2. 5.85
3. 4.35
4. 5.18
\(4HCl + MnO_2 \rightarrow 2H_2O + MnCl_2 + Cl_2\)
Amount(in g) of manganese dioxide that reacts with 7.3 g of HCl is:
(Atomic weight of Mn is 55)
1. 0.23
2. 5.85
3. 4.35
4. 5.18
Subtopic: Equation Based Problem |
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Which one of the following samples of gases contains the most particles?
All gases are at 0 °C and 1 atm pressure when 1 mole of gas has a volume of 22.4 L.
[Relative atomic mass, Ar : H = 1, He = 4, C = 12, O = 16, Cl = 35.5]
1. 33.6 L of chlorine gas
2. 66.0 g of carbon dioxide gas
3. 22.4 L of hydrogen gas
4. 10.0 g of helium gas
All gases are at 0 °C and 1 atm pressure when 1 mole of gas has a volume of 22.4 L.
[Relative atomic mass, Ar : H = 1, He = 4, C = 12, O = 16, Cl = 35.5]
1. 33.6 L of chlorine gas
2. 66.0 g of carbon dioxide gas
3. 22.4 L of hydrogen gas
4. 10.0 g of helium gas
Subtopic: Moles, Atoms & Electrons |
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Calculate the approximate mass of \(CO_2\) produced when 1 gm of butane \((C_4H_{10})\) is burned with
an excess of \(O_2\) to form \(CO_2\).
an excess of \(O_2\) to form \(CO_2\).
| 1. | 1 g | 2. | 2 g |
| 3. | 3 g | 4. | 4 g |
Subtopic: Equation Based Problem |
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Which, of the following, laws of chemical combination is followed by \(N_2O~, NO \) and \(N_2O_3\) ?
1. Law of conservation of mass
2. Law of multiple proportions
3. Law of constant proportions
4. Gay Lussac's law of constant volume
1. Law of conservation of mass
2. Law of multiple proportions
3. Law of constant proportions
4. Gay Lussac's law of constant volume
Subtopic: Introduction |
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For the reaction, \(2A+B\xrightarrow{~~~~~~~~}3C,8\) moles of \(A\) reacts with \(5\) moles of \(B\) to form \(C.\)
Calculate the maximum number of moles that are formed.
1. \(13\) mole
2. \(15\) mole
3. \(12\) mole
4. \(8\) mole
Calculate the maximum number of moles that are formed.
1. \(13\) mole
2. \(15\) mole
3. \(12\) mole
4. \(8\) mole
Subtopic: Limiting Reagent |
77%
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An aqueous solution of urea containing 18 g of urea in 1500 cm3 of the solution has a density of 1.052 g/cm3. If the molecular weight of urea is 60, then the molality of the solution is-
1. 0.2
2. 0.192
3. 0.064
4. 1.2
Subtopic: Concentration Based Problem |
70%
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The NaNO3 weighed out to make 50 mL of an aqueous solution containing 70.0 mg Na+ per mL is-
(Rounded off to the nearest integer) [Given: Atomic weight in g mol–1 – Na: 23; N: 14; O: 16]
1. 13 g
2. 26 g
3. 18 g
4. 22 g
Subtopic: Concentration Based Problem |
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A solution is prepared by adding 2 g of substance A to 18 g of water. The mass percent of the solute is-
1. 20%
2. 10%
3. 15%
4. 18%
Subtopic: Concentration Based Problem |
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NEET 2023 - Target Batch - Aryan Raj Singh
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