Q. No.Which of the following statements is correct about the reaction is given below?
| 1. | Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass |
| 2. | Total mass of reactants = total mass of product, therefore, law of multiple proportions is followed |
| 3. | Amount of Fe2O3 can be increased by taking any one of the reactants (iron or oxygen) in excess. |
| 4. | Amount of Fe2O3 produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess. |
Subtopic: Limiting Reagent |
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What is the total volume of gases present after the completion of the reaction between 150 cm3 of F2 and 100 cm3 of Cl2?
3F2 (g) + Cl 2(g) → 2ClF3 (g)
(assuming the reaction occurs at constant temperature and pressure)
1. 250 cm3
2. 150 cm3
3. 350 cm3
4. 200 cm3
3F2 (g) + Cl 2(g) → 2ClF3 (g)
(assuming the reaction occurs at constant temperature and pressure)
1. 250 cm3
2. 150 cm3
3. 350 cm3
4. 200 cm3
Subtopic: Limiting Reagent | Introduction |
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To produce 20 moles of ammonia via Haber's process, how many moles of hydrogen molecules are required?
| 1. | 40 mol | 2. | 10 mol |
| 3. | 20 mol | 4. | 30 mol |
Subtopic: Limiting Reagent | Equation Based Problem |
80%
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NEET - 2019
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When one mole ammonia and one mole oxygen are taken:
1. Oxygen is completely consumed
2. Ammonia is completely consumed
3. Both (1) and (2) are correct
4. None of the above options is correct
Subtopic: Limiting Reagent |
67%
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AIPMT - 1998
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The amount of Zinc (atomic weight = 65) necessary to produce 224 mL of H2 (at STP) by the reaction with dilute sulphuric acid will be:
| 1. | 0.65 g | 2. | 7.6 g |
| 3. | 6.5 g | 4. | 8.5 g |
Subtopic: Limiting Reagent |
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20 ml of nitric oxide combines with 10 ml of oxygen at STP to give NO2. The final volume will be:
1. 30 ml
2. 20 ml
3. 10 ml
4. 40 ml
1. 30 ml
2. 20 ml
3. 10 ml
4. 40 ml
Subtopic: Limiting Reagent |
63%
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Consider the following reaction:
\(2ZnS\,+\,3O_2\) → \(2ZnO \,+\,2SO_2 \)
If 97.5 grams of zinc sulphide undergo this reaction with 32 grams of oxygen gas, the limiting reagent will be:
(Given: Molar mass ZnS = 97.5 g/mol)
1. ZnS
2. O2
3. ZnO
4. SO2
\(2ZnS\,+\,3O_2\) → \(2ZnO \,+\,2SO_2 \)
If 97.5 grams of zinc sulphide undergo this reaction with 32 grams of oxygen gas, the limiting reagent will be:
(Given: Molar mass ZnS = 97.5 g/mol)
1. ZnS
2. O2
3. ZnO
4. SO2
Subtopic: Limiting Reagent |
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10 gm carbon reacts with 100 gm \(Cl_2\) to form \(CCl_4\). The maximum weight of \(CCl_4\) formed will be:
1. 128 gm
2. 94.22 gm
3. 108.45 gm
4. 54.22 gm
1. 128 gm
2. 94.22 gm
3. 108.45 gm
4. 54.22 gm
Subtopic: Limiting Reagent |
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The elements A (atomic weight = 75) and B (atomic weight = 32) combine to form a compound X. If 3 moles of B combine with 2 moles of A to produce 1 mole of X, the weight of 5 moles of X will be:
1. 246 gm
2. 1230 amu
3. 1.23 kg
4. None of the above
1. 246 gm
2. 1230 amu
3. 1.23 kg
4. None of the above
Subtopic: Limiting Reagent |
51%
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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 |
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