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Q. No.Calculate the mass of 95% pure CaCO3 that will be required to neutralize 50 mL of 0.5 M HCl solution according to the following reaction.
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + 2H2O(l)
[Calculate up to the second place of decimal point]
1.
9.50 g
2.
1.25 g
3.
1.32 g
4.
3.65 g
Subtopic: Equation Based Problem |
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NEET - 2022
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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%
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NEET - 2022
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Two elements A & B form two different compounds A2B & AB3. If 0.15 mole of both compounds have equal weight then what is the ratio of the molar atomic mass of A & B?
1. 2 : 1
2. 6 : 4
3. 1 : 2
4. 4 : 6
1. 2 : 1
2. 6 : 4
3. 1 : 2
4. 4 : 6
Subtopic: Moles, Atoms & Electrons |
59%
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If 0.02 moles of H2SO4 are present in 1 litre of solution from which 50% solution is taken out and again diluted up to 1 litre by adding water. Further, if 0.01 moles of H2SO4 are added, then the total millimoles of H2SO4 in the resulting solution will be:
1. 10
2. 5
3. 20
4. 15
1. 10
2. 5
3. 20
4. 15
Subtopic: Concentration Based Problem |
55%
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The number of moles of water present in a spherical water droplet of radius 1.0 cm are:
[Given: Density of water in the droplet = 1.0 g cm–3]
1. \( \dfrac{\pi}{18} \)
2. \( \dfrac{2\pi}{27} \)
3. \(24\pi\)
4. \( \dfrac{2\pi}{9} \)
[Given: Density of water in the droplet = 1.0 g cm–3]
1. \( \dfrac{\pi}{18} \)
2. \( \dfrac{2\pi}{27} \)
3. \(24\pi\)
4. \( \dfrac{2\pi}{9} \)
Subtopic: Introduction |
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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 |
51%
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The mass of a 2.5 mL solution (the density of the solution is 2.15 g/mL) in the correct significant figures is:
| 1. | 5375 × 10–3 g | 2. | 5.4 g |
| 3. | 5.38 g | 4. | 53.75 g |
Subtopic: Introduction |
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NEET - 2022
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9.8 gm \(KClO_3 \) is decomposed and the weight loss was observed to be 0.384 gm. The percentage of \(KClO_3\) decomposed is:
1. 10%
2. 20%
3. 40%
4. 100%
1. 10%
2. 20%
3. 40%
4. 100%
Subtopic: Equation Based Problem |
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The molarity of \(NaNO_3 \) solution (molecular weight of \(NaNO_3\) = 85) is 1M. The density of the solution is 1.25 gm/ml. The molality of the solution, approximately, will be:
1. 0.80
2. 0.86
3. 0.96
4. 1
1. 0.80
2. 0.86
3. 0.96
4. 1
Subtopic: Concentration Based Problem |
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In an experiment, it showed that 10 mL of 0.05 M solution of chloride required 10 mL of 0.1 M solution of AgNO3. Which of the following will be the formula of the chloride (X stands for the symbol of the element other than chlorine)?
1. X2Cl2
2. XCl2
3. XCl4
4. X2Cl
1. X2Cl2
2. XCl2
3. XCl4
4. X2Cl
Subtopic: Equation Based Problem |
70%
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NEET - 2013
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