Jamb chemistry 1, what mass of water is produced when 8.0g of hydrogen reacts with excess oxygen
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
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Let's solve this chemistry problem.
Step 1: Write the balanced chemical equation.
The reaction between hydrogen and oxygen produces water.
2H₂(g) + O₂(g) → 2H₂O(l)
Step 2: Calculate the moles of hydrogen (H₂).
We'll use the molar masses: H = 1 g/mol, O = 16 g/mol.
Molar mass of H₂ = 2 × 1 g/mol = 2 g/mol
Moles of H₂ = Mass / Molar mass
Moles of H₂ = 8.0 g / 2 g/mol
Moles of H₂ = 4.0 mol
Step 3: Use the mole ratio from the balanced equation to find moles of water.
From the balanced equation, 2 moles of H₂ produce 2 moles of H₂O. This is a 1:1 mole ratio.
Moles of H₂O = Moles of H₂
Moles of H₂O = 4.0 mol
Step 4: Calculate the mass of water (H₂O) produced.
Molar mass of H₂O = (2 × 1 g/mol) + 16 g/mol = 18 g/mol
Mass of H₂O = Moles × Molar mass
Mass of H₂O = 4.0 mol × 18 g/mol
Mass of H₂O = 72 g
The mass of water produced is 72 g.
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