In the equation

Question

2H2+1O2→→2H2O

if you change the 2H2 to 3H2 molecules and balance the equation, identify which statement is correct?

(1 point)
Responses

The result of the equation will be the same.
The result of the equation will be the same.

It is not possible to produce water without leftover molecules.
It is not possible to produce water without leftover molecules.

Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules.
Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules.

The equation will produce three molecules of water.
The equation will produce three molecules of water.

Answer 1

To balance the modified equation where you change the 2H2 to 3H2:

Starting with:
3H2 + O2 → ?

We need to balance the hydrogen and oxygen atoms. The reaction now has 3 molecules of H2, which gives us 6 hydrogen atoms. To balance this with oxygen, we need 3 water molecules (H2O) since each water molecule contains 2 hydrogen atoms:

So the balanced equation becomes:
3H2 + 1.5O2 → 3H2O

Since we often express coefficients as whole numbers, we can multiply the entire equation by 2 to eliminate the fraction:
6H2 + 3O2 → 6H2O

Now, let's evaluate the given statements based on the balanced equation:

1. The result of the equation will be the same.

   • This is incorrect because the result changes to 6 water molecules.

2. It is not possible to produce water without leftover molecules.

   • This is incorrect for the balanced equation since we have a complete reaction with no leftover reactants.

3. Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules.

   • This is incorrect because for the new equation, each oxygen molecule combines with 3 hydrogen molecules.

4. The equation will produce three molecules of water.

   • This is incorrect after balancing; the equation produces six molecules of water.

Considering the analysis above, none of the provided statements are correct when adjusting for the new balanced equation. However, the closest statement to the truth regarding the balanced reaction is that oxygen molecules are consumed completely in producing water.

If I must select from these statements, option #3 has a partial truth because typically we balance equations for two hydrogen molecules per oxygen molecule, but here, it produced more than suggested. To clarify, there are no leftover molecules in fully balanced reactions in its proper context.

In summary, none of the statements wholly captures the chemical changes without a proper perspective of a rebalanced output; in the rebalanced scenario, you must acknowledge that 3H2 utilizes 1.5O2 to form 3H2O; hence, "each oxygen molecule interacts with slightly nuanced ratios."