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Answer :
The amount of water formed when 10.0 g of hydrogen is combined with 100.0 g of oxygen and burned is 178.2 g, and this is the right answer.
How many grammes of hydrogen need 10.0 grammes of oxygen to react?
water volume produced as a result of the given amount of hydrogen and oxygen reacting. - As a result, 10 g of hydrogen and 80 g of oxygen must react for 112 L of water to be produced.
We must first formulate the balanced chemical equation for the reaction of oxygen and hydrogen in order to solve this issue:
2H2 + O2 → 2H2O
To convert grammes to moles, we can utilise each element's molar mass:
Number of moles of H2 = 10.0 g / 2.02 g/mol = 4.95 mol
Number of moles of O2 = 100.0 g / 32.00 g/mol = 3.125 mol
The amount of water produced can be determined using the number of moles of H2:
Number of moles of H2O = 2 x (4.95 mol)
= 9.90 mol
Finally, using the molar mass of water, we can translate the quantity of moles of water into grammes:
Mass of H2O = 9.90 mol x 18.02 g/mol
= 178.2 g
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