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Please answer!
See the above image
According to the Law of mass of conservation,
Mass of Products = Mass of Reactants
Then why it doesn't followed the same in above reaction given in the picture?
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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 H2as 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 H2and 50 ml O2 to make 100 ml H2O as long as they are at the same temperature and pressure.
good evening _________✌️✌️✌️✌️
_______________________
_____________
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 H2as 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 H2and 50 ml O2 to make 100 ml H2O as long as they are at the same temperature and pressure.
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