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Q. No.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
Subtopic: Moles, Atoms & Electrons |
Level 3: 35%-60%
Hints
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 a 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. |
Subtopic: Introduction |
52%
Level 3: 35%-60%
Hints
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 |
75%
Level 2: 60%+
Hints
Which one of the following samples of gases contains the most particles? If all the 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
[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 |
Level 4: Below 35%
Hints
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 \(CO_2\).
| 1. | 1 g | 2. | 2 g |
| 3. | 3 g | 4. | 4 g |
Subtopic: Equation Based Problem |
67%
Level 2: 60%+
Hints
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 |
79%
Level 2: 60%+
Hints
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.
Calculate the maximum number of moles that are formed.
| 1. | \(13\) moles | 2. | \(15\) moles |
| 3. | \(12\) moles | 4. | \(8\) moles |
Subtopic: Limiting Reagent |
78%
Level 2: 60%+
Hints
An aqueous solution contains 18 g of urea in 1500 cm³ of solution.
If the density of the solution is 1.052 g cm⁻³ and the molar mass of urea is 60 g mol⁻¹,
calculate the molality of the solution.
1. 0.2
2. 0.192
3. 0.064
4. 1.2
Subtopic: Concentration Based Problem |
67%
Level 2: 60%+
Hints
Find the mass of NaNO₃ required to prepare 50 mL of aqueous solution containing 70.0 mg Na⁺ per mL.
(Round off to the nearest integer.
Given: Na = 23, N = 14, O = 16)
| 1. | 13 g | 2. | 26 g |
| 3. | 18 g | 4. | 22 g |
Subtopic: Concentration Based Problem |
54%
Level 3: 35%-60%
Hints
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 |
85%
Level 1: 80%+
Hints
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