To balance the modified equation where you have 3H₂ instead of 2H₂, we start with:
3H₂ + O₂ → H₂O
Balancing the equation, we need to ensure that the number of atoms on both sides remains the same.
- We start with 3 hydrogen (H) from 3 molecules of H₂.
- Since each molecule of water (H₂O) contains 2 hydrogen atoms, to balance the 3 hydrogen atoms, we need to produce 1.5 molecules of water, which isn't practical since we cannot have half a molecule.
To balance it fully, if we use 3 molecules of H₂, the balanced equation would be:
3H₂ + 1.5O₂ → 3H₂O
This means if we're strictly balancing the reaction, we would need 1.5 molecules of O₂, which would imply that we still do not achieve whole molecules on both sides without leftover.
Now evaluating the options given:
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"Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules." - This is incorrect in this scenario.
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"It is not possible to produce water without leftover molecules." - This could be considered correct in this altered context with 3H₂, as it leads to half a molecule of O₂.
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"The equation will produce three molecules of water." - This is also correct in that if balanced, we would yield three molecules of water, but we do have the half O₂ issue.
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"The result of the equation will be the same." - This seems incorrect, as changing the amount of H₂ alters the balance.
Thus, the most accurate statement from the choices is:
"It is not possible to produce water without leftover molecules."