Answer :
To determine which statement is true for the given reaction:
[tex]\[ H_2 + O_2 \longrightarrow H^+ + O^{2-} \][/tex]
we must check the balance of both the number of atoms on each side and their oxidation states. Here is a step-by-step analysis:
### Step 1: Check the Balance of Atoms
- Left side:
- \(H_2\): 2 hydrogen atoms
- \(O_2\): 2 oxygen atoms
- Right side:
- \(H^+\): 1 hydrogen ion (1 hydrogen atom)
- \(O^{2-}\): 1 oxygen ion (1 oxygen atom)
So, we have:
- Hydrogen atoms on the left: 2
- Oxygen atoms on the left: 2
- Hydrogen atoms on the right: 1
- Oxygen atoms on the right: 1
Clearly, the number of hydrogen and oxygen atoms on the left does not equal the number of these atoms on the right. Therefore, the reaction is not balanced for the number of atoms.
### Step 2: Check the Balance of Oxidation States
- Left side:
- \(H_2\): Each hydrogen atom in \(H_2\) has an oxidation state of 0.
- Total for \(H_2\): \(2 \times 0 = 0\)
- \(O_2\): Each oxygen atom in \(O_2\) has an oxidation state of 0.
- Total for \(O_2\): \(2 \times 0 = 0\)
- Right side:
- \(H^+\): The hydrogen ion has an oxidation state of +1.
- \(O^{2-}\): The oxygen ion has an oxidation state of -2.
So, we have:
- Oxidation state sum on the left: \(0 + 0 = 0\)
- Oxidation state sum on the right: \(+1 + (-2) = -1\)
Clearly, the total oxidation state on the left does not equal the total oxidation state on the right. Therefore, the reaction is not balanced for oxidation state.
### Conclusion
Given the analyses above, the reaction is neither balanced for the number of atoms nor for oxidation state. Therefore, the true statement is:
[tex]\[ \text{It is not balanced for oxidation state or for number of atoms.} \][/tex]
[tex]\[ H_2 + O_2 \longrightarrow H^+ + O^{2-} \][/tex]
we must check the balance of both the number of atoms on each side and their oxidation states. Here is a step-by-step analysis:
### Step 1: Check the Balance of Atoms
- Left side:
- \(H_2\): 2 hydrogen atoms
- \(O_2\): 2 oxygen atoms
- Right side:
- \(H^+\): 1 hydrogen ion (1 hydrogen atom)
- \(O^{2-}\): 1 oxygen ion (1 oxygen atom)
So, we have:
- Hydrogen atoms on the left: 2
- Oxygen atoms on the left: 2
- Hydrogen atoms on the right: 1
- Oxygen atoms on the right: 1
Clearly, the number of hydrogen and oxygen atoms on the left does not equal the number of these atoms on the right. Therefore, the reaction is not balanced for the number of atoms.
### Step 2: Check the Balance of Oxidation States
- Left side:
- \(H_2\): Each hydrogen atom in \(H_2\) has an oxidation state of 0.
- Total for \(H_2\): \(2 \times 0 = 0\)
- \(O_2\): Each oxygen atom in \(O_2\) has an oxidation state of 0.
- Total for \(O_2\): \(2 \times 0 = 0\)
- Right side:
- \(H^+\): The hydrogen ion has an oxidation state of +1.
- \(O^{2-}\): The oxygen ion has an oxidation state of -2.
So, we have:
- Oxidation state sum on the left: \(0 + 0 = 0\)
- Oxidation state sum on the right: \(+1 + (-2) = -1\)
Clearly, the total oxidation state on the left does not equal the total oxidation state on the right. Therefore, the reaction is not balanced for oxidation state.
### Conclusion
Given the analyses above, the reaction is neither balanced for the number of atoms nor for oxidation state. Therefore, the true statement is:
[tex]\[ \text{It is not balanced for oxidation state or for number of atoms.} \][/tex]
