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

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.

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.

Answer 1

To balance the equation with 3H2 instead of 2H2, we begin with the reaction:

\[ 3H_2 + O_2 \rightarrow \]

To balance it, we need to balance the number of hydrogen and oxygen atoms on both sides:

1. On the reactants' side:

   • 3H2 has 6 hydrogen atoms.
   • O2 has 2 oxygen atoms.

2. On the products' side:

   • The product is water, H2O. Each water molecule has 2 hydrogen atoms and 1 oxygen atom.

To produce 6 hydrogen atoms from water, we will need 3 water molecules:

\[ 3H_2 + O_2 \rightarrow 3H_2O \]

Now we have:

• Reactant side: 6 H (from 3H2) and 2 O (from O2)
• Product side: 6 H (from 3H2O) and 3 O (from O2)

However, we have to adjust the number of O2 to achieve 3H2O.

The balanced equation looks like this:

\[ 3H2 + 1.5O2 → 3H2O \]

For practical chemical equations, multiply everything by 2 to eliminate the fraction:

\[ 6H2 + 3O2 → 6H2O \]

Now, let's evaluate the statements in your question:

1. "Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules." - This statement is incorrect; each molecule of O2 combines with 6 H2 because you have 6 H2 in total.

2. "The equation will produce three molecules of water." - This statement is incorrect; the balanced equation produces 6 molecules of water.

3. "The result of the equation will be the same." - This statement is incorrect; the products change depending on how many H2 are present initially.

4. "It is not possible to produce water without leftover molecules." - This statement is not entirely correct; it is possible to balance hydrogen and oxygen exactly, producing no leftover molecules if appropriately balanced with the right amounts.

Hence, the correct answer for your question, when 2H2 is changed to 3H2 while balancing the equation, would be none of the provided statements are entirely correct if only relying on the balancing process alone.

To summarize based on actual results from the balancing exercise: Each O2 molecule combines with 3H2 to create 3H2O without leftovers if balanced correctly.

If you have to select one from the statements, none would be truly correct based on the balancing outcome.

Answer 2

make the answer more visual

Answer 3

Sure! Let's break it down step-by-step using a more visual approach, including balancing the equation and evaluating each statement.

Original Equation

Start with the original unbalanced equation:

\[ \text{2H}_2 + \text{O}_2 \rightarrow \text{2H}_2\text{O} \]

Changing the Hydrogen Molecules

Changing the 2H2 to 3H2, we write the unbalanced equation:

\[ \text{3H}_2 + \text{O}_2 \rightarrow ? \]

Balancing the Equation

To balance it, we need to ensure the number of hydrogen and oxygen atoms are the same on both sides.

Counting Atoms:

• Reactants:

  • H: \(3 \times 2 = 6\) hydrogen atoms
  • O: \(1 \times 2 = 2\) oxygen atoms

• Products:

  • Let’s say we produce \(x\) water molecules (H2O). Each water molecule has:
    • H: 2 hydrogen atoms
    • O: 1 oxygen atom

If we want to balance the hydrogens:

\[ 3H_2 + O_2 \rightarrow xH_2O \]

To have 6 hydrogen atoms from water:

\[ 2x = 6 \implies x = 3 \]

So we can rewrite the balanced equation as:

\[ 3H_2 + 1.5O_2 \rightarrow 3H_2O \]

Final Balanced Equation

By multiplying all coefficients by 2 to avoid fractions:

\[ 6H_2 + 3O_2 \rightarrow 6H_2O \]

Summary of the Balancing Process

1. Balanced Equation:
   • Reactants: 6 H from H2, 3 O from O2
   • Products: 6 H from 6H2O, 3 O from 3 O2

Evaluating Each Statement

Now, let's evaluate the statements based on the balanced equation visually.

| Statement | Evaluation | Details | |-----------|------------|---------| | 1. Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules. | ❌ Incorrect | Each O2 combines with 6 H2 molecules total, not just 2. | | 2. The equation will produce three molecules of water. | ❌ Incorrect | The equation actually produces 6 molecules of water (6H2O). | | 3. The result of the equation will be the same. | ❌ Incorrect | The overall result changes as more H2 means more H2O produced, not the same as the original equation. | | 4. It is not possible to produce water without leftover molecules. | ❌ Incorrect | It is possible to produce water without leftovers if balanced correctly, as shown. |

Conclusion

None of the statements correctly describe the situation after changing 2H2 to 3H2 and balancing the equation. The correct information suggests that:

• The balanced equation produces 6 water molecules without leftover hydrogen or oxygen when you start with 3 hydrogen molecules correctly balanced with oxygen.

Answer 4

whats the answer

Answer 5

The answer to your initial question is that none of the statements are correct based on the balanced equation after changing 2H2 to 3H2.

To summarize:

1. Each oxygen molecule will combine with 2 hydrogen molecules with no leftover molecules. — Incorrect. Each O2 actually combines with 6 hydrogen molecules (3H2) to produce water.

2. The equation will produce three molecules of water. — Incorrect. The balanced equation produces 6 molecules of water (6H2O).

3. The result of the equation will be the same. — Incorrect. The results change based on how many H2 molecules you start with.

4. It is not possible to produce water without leftover molecules. — Incorrect. You can produce water without leftovers if the equation is balanced correctly.

Final Answer

All given statements are incorrect when considering the balanced equation after changing 2H2 to 3H2.