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10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be: [2009]
- a)3 mol
- b)4 mol
- c)1 mol
- d)2 mol
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and ...
In this reaction oxygen is the limiting agent.
Hence amount of H2O produced depends on the amount of O2 taken 0.5 mole of O2 gives H2O = 1 mol
∴ 2 mole of O2 gives H2O = 4 mol
Hence amount of H2O produced depends on the amount of O2 taken 0.5 mole of O2 gives H2O = 1 mol
∴ 2 mole of O2 gives H2O = 4 mol
Most Upvoted Answer
10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and ...
**Balanced Chemical Equation:**
To determine the amount of water produced in the reaction, we first need to write the balanced chemical equation for the reaction between hydrogen and oxygen:
2H2 + O2 -> 2H2O
This equation shows that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
**Calculating Moles:**
To calculate the moles of hydrogen and oxygen given in the question, we can use the formula:
moles = mass / molar mass
The molar mass of hydrogen (H2) is 2 g/mol, and the molar mass of oxygen (O2) is 32 g/mol.
Moles of hydrogen = 10 g / 2 g/mol = 5 mol
Moles of oxygen = 64 g / 32 g/mol = 2 mol
**Limiting Reactant:**
The reactant that is completely consumed in a reaction is called the limiting reactant. The amount of product formed is determined by the limiting reactant.
In this case, hydrogen is present in excess (5 moles) while oxygen is the limiting reactant (2 moles). Therefore, the amount of water produced will be determined by the moles of oxygen.
**Amount of Water Produced:**
From the balanced equation, we know that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
Since there are 2 moles of oxygen, the amount of water produced will be:
2 moles of oxygen * 2 moles of water / 1 mole of oxygen = 4 moles of water
Therefore, the correct answer is option 'B' - 4 mol.
To determine the amount of water produced in the reaction, we first need to write the balanced chemical equation for the reaction between hydrogen and oxygen:
2H2 + O2 -> 2H2O
This equation shows that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
**Calculating Moles:**
To calculate the moles of hydrogen and oxygen given in the question, we can use the formula:
moles = mass / molar mass
The molar mass of hydrogen (H2) is 2 g/mol, and the molar mass of oxygen (O2) is 32 g/mol.
Moles of hydrogen = 10 g / 2 g/mol = 5 mol
Moles of oxygen = 64 g / 32 g/mol = 2 mol
**Limiting Reactant:**
The reactant that is completely consumed in a reaction is called the limiting reactant. The amount of product formed is determined by the limiting reactant.
In this case, hydrogen is present in excess (5 moles) while oxygen is the limiting reactant (2 moles). Therefore, the amount of water produced will be determined by the moles of oxygen.
**Amount of Water Produced:**
From the balanced equation, we know that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
Since there are 2 moles of oxygen, the amount of water produced will be:
2 moles of oxygen * 2 moles of water / 1 mole of oxygen = 4 moles of water
Therefore, the correct answer is option 'B' - 4 mol.
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10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be: [2009]a)3 molb)4 molc)1 mold)2 molCorrect answer is option 'B'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be: [2009]a)3 molb)4 molc)1 mold)2 molCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be: [2009]a)3 molb)4 molc)1 mold)2 molCorrect answer is option 'B'. Can you explain this answer?.
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