Q. No.Which of the following statements about the reaction given below is correct?
| 1. | Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows the law of conservation of mass |
| 2. | Total mass of reactants = total mass of product, therefore, the law of multiple proportions is followed |
| 3. | The amount of Fe2O3 can be increased by taking any one of the reactants (iron or oxygen) in excess. |
| 4. | The 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 1 mole of ammonia (NH₃) reacts with 1 mole of oxygen (O₂), which of the following outcomes occurs regarding the consumption of the reactants?
| 1. | Oxygen is completely consumed. |
| 2. | Ammonia is completely consumed. |
| 3. | Both oxygen (O₂) and ammonia (NH₃) are completely consumed |
| 4. | Neither oxygen (O₂) nor ammonia (NH₃) is completely consumed. |
Subtopic: Limiting Reagent |
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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 |
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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 |
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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.
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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