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Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)?
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Consider the equation 2H2 + O2=2H2O.What mass of water will be produce...
Calculating the mass of water produced:
To calculate the mass of water produced when 0.1g of hydrogen reacts with oxygen, we first need to determine the limiting reactant in the reaction.
Step 1: Determine the limiting reactant:
- Calculate the number of moles of hydrogen:
- 0.1g H2 * (1 mol H2 / 2g H2) = 0.05 mol H2
- Calculate the number of moles of oxygen needed for complete reaction:
- From the balanced equation, 2 moles of H2 react with 1 mole of O2
- Therefore, 0.05 mol H2 would require 0.025 mol O2
Step 2: Calculate the mass of water produced:
- From the balanced equation, 2 moles of H2 produce 2 moles of H2O
- Therefore, 0.05 mol H2 would produce 0.05 mol H2O
- Calculate the mass of water produced:
- Mass = number of moles * molar mass
- Mass of water = 0.05 mol * 18 g/mol = 0.9 g
Therefore, when 0.1g of hydrogen reacts with oxygen, the mass of water produced will be 0.9g. This calculation assumes that hydrogen is the limiting reactant, and the reaction goes to completion.
To calculate the mass of water produced when 0.1g of hydrogen reacts with oxygen, we first need to determine the limiting reactant in the reaction.
Step 1: Determine the limiting reactant:
- Calculate the number of moles of hydrogen:
- 0.1g H2 * (1 mol H2 / 2g H2) = 0.05 mol H2
- Calculate the number of moles of oxygen needed for complete reaction:
- From the balanced equation, 2 moles of H2 react with 1 mole of O2
- Therefore, 0.05 mol H2 would require 0.025 mol O2
Step 2: Calculate the mass of water produced:
- From the balanced equation, 2 moles of H2 produce 2 moles of H2O
- Therefore, 0.05 mol H2 would produce 0.05 mol H2O
- Calculate the mass of water produced:
- Mass = number of moles * molar mass
- Mass of water = 0.05 mol * 18 g/mol = 0.9 g
Therefore, when 0.1g of hydrogen reacts with oxygen, the mass of water produced will be 0.9g. This calculation assumes that hydrogen is the limiting reactant, and the reaction goes to completion.
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Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)?
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Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)? for UPSC 2025 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)? covers all topics & solutions for UPSC 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)?.
Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)? for UPSC 2025 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)? covers all topics & solutions for UPSC 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider the equation 2H2 + O2=2H2O.What mass of water will be produced,if 0.1gm hydrogen is completely reacting with oxygen (atomic mass: H=1,O=16)?.
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