How does 100 ml of hydrogen combine with 50 ml of oxygen?
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Answer:
as H and 0 combine in the ratio 2 : 1 therefore 100 ml / 50 ml = 2
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Answer:
Let's look at the chemical equation in question.
2H2 + O2 ==> 2H2O
As can be seen from the BALANCED equation, it takes twice as much H2 as it does O2 to make water. And the amount of water is equal to the amount of H2 and equal to half the amount of O2. The "amounts" can be in mls or moles as long as both H2 and O2 are being measured at the same temperature and pressure. So, this DOES NOT violate the law of conservation of mass.
Take 2 moles H2 and 1 mole of O2 to make 2 moles of H2O
Mass of reactants = 2 x 2 = 4 g + 1 x 32 = 32 g = 36 g total mass of reactants
Mass of product = 2 x 18 = 36 g total mass of product
The same will be true with 100 ml H2 and 50 ml O2 to make 100 ml H2O as long as they are at the same temperature and pressure.
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