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A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce that
- a)The atomic weight of the metal is 8
- b)The atomic weight of the metal is 4
- c)The equivalent weight of the metal is 4
- d)The equivalent weight of the metal is 8
Correct answer is option 'C'. Can you explain this answer?
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A metal oxide is reduced by heating it in a stream of hydrogen. It is ...
So the equivalent weight of the metal is 4.
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A metal oxide is reduced by heating it in a stream of hydrogen. It is ...
Given information:
- A metal oxide is reduced by heating it in a stream of hydrogen.
- After complete reduction, 3.15 g of the oxide yields 1.05 g of the metal.
To deduce the equivalent weight of the metal:
To deduce the equivalent weight of the metal, we need to understand the concept of equivalent weight.
Equivalent weight:
The equivalent weight of a substance is the weight in grams that is chemically equivalent to one mole of a specific reagent or is equal to the ratio of the molecular weight to the valence.
Steps to determine the equivalent weight:
1. Calculate the number of moles of the metal and the oxide.
2. Use the stoichiometry of the reaction to determine the mole ratio of the metal to the oxide.
3. Calculate the equivalent weight of the metal using the mole ratio.
Calculation:
1. Calculate the number of moles of the metal and the oxide:
- The number of moles of the oxide = 3.15 g / molar mass of the oxide
- The number of moles of the metal = 1.05 g / molar mass of the metal
2. Use the stoichiometry of the reaction to determine the mole ratio of the metal to the oxide:
- The balanced chemical equation for the reduction of the metal oxide can give us the mole ratio.
Example:
MxOy + zH2 → xM + y/2H2O
From the equation, we can see that for every x moles of the metal (M), y/2 moles of water (H2O) are formed. Therefore, the mole ratio of the metal to the oxide is x:y/2.
3. Calculate the equivalent weight of the metal using the mole ratio:
- The equivalent weight of the metal = molar mass of the metal / (x:y/2)
Conclusion:
Based on the given information, we can deduce that the equivalent weight of the metal is 4. This is because the ratio of the mass of the metal to the mass of the oxide is 1:3, indicating that the mole ratio of the metal to the oxide is 1:3/2 or 2:3. Therefore, the equivalent weight of the metal can be calculated as the molar mass of the metal divided by the mole ratio, which gives a value of 4.
- A metal oxide is reduced by heating it in a stream of hydrogen.
- After complete reduction, 3.15 g of the oxide yields 1.05 g of the metal.
To deduce the equivalent weight of the metal:
To deduce the equivalent weight of the metal, we need to understand the concept of equivalent weight.
Equivalent weight:
The equivalent weight of a substance is the weight in grams that is chemically equivalent to one mole of a specific reagent or is equal to the ratio of the molecular weight to the valence.
Steps to determine the equivalent weight:
1. Calculate the number of moles of the metal and the oxide.
2. Use the stoichiometry of the reaction to determine the mole ratio of the metal to the oxide.
3. Calculate the equivalent weight of the metal using the mole ratio.
Calculation:
1. Calculate the number of moles of the metal and the oxide:
- The number of moles of the oxide = 3.15 g / molar mass of the oxide
- The number of moles of the metal = 1.05 g / molar mass of the metal
2. Use the stoichiometry of the reaction to determine the mole ratio of the metal to the oxide:
- The balanced chemical equation for the reduction of the metal oxide can give us the mole ratio.
Example:
MxOy + zH2 → xM + y/2H2O
From the equation, we can see that for every x moles of the metal (M), y/2 moles of water (H2O) are formed. Therefore, the mole ratio of the metal to the oxide is x:y/2.
3. Calculate the equivalent weight of the metal using the mole ratio:
- The equivalent weight of the metal = molar mass of the metal / (x:y/2)
Conclusion:
Based on the given information, we can deduce that the equivalent weight of the metal is 4. This is because the ratio of the mass of the metal to the mass of the oxide is 1:3, indicating that the mole ratio of the metal to the oxide is 1:3/2 or 2:3. Therefore, the equivalent weight of the metal can be calculated as the molar mass of the metal divided by the mole ratio, which gives a value of 4.
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A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer?
Question Description
A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer?.
A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer?.
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A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer?, a detailed solution for A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? has been provided alongside types of A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 3.15 g of the oxide has yielded 1.05 g of the metal. We may deduce thata)The atomic weight of the metal is 8b)The atomic weight of the metal is 4c)The equivalent weight of the metal is 4d)The equivalent weight of the metal is 8Correct answer is option 'C'. Can you explain this answer? tests, examples and also practice NEET tests.
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