solve step by step:Methanol gas, CH3OH(g), can be manufactured industrially by the catalytic hydrogenation of carbon monoxide, CO(g), as represented by the following equation.

CO(g) + 2 H2(g) → CH3OH(g)

1. In the reaction represented above, hydrogen gas acts as the agent and the oxidation number for carbon in CO(g)

The statement above is best completed by the answers in row.

Row

i

ii

oxidizing

increases

oxidizing

decreases

reducing

decreases

reducing

increases

2. The total number of electrons transferred in the industrial production of methanol

2

4

6

8

To solve this problem step-by-step, we need to determine the roles of the reactants and the changes in oxidation numbers during the reaction.

### Step 1: Determine the Oxidation Numbers

#### CO(g) (Carbon Monoxide)
- The oxidation number of oxygen in CO is -2.
- Let \( x \) be the oxidation number of carbon.

For the molecule CO, the equation is:
\[ x + (-2) = 0 \]
\[ x = +2 \]

So, the oxidation number for carbon in CO(g) is +2.

#### CH₃OH(g) (Methanol)
- Hydrogen has an oxidation number of +1.
- Oxygen has an oxidation number of -2.
- Let \( x \) be the oxidation number of carbon.

For the molecule CH₃OH, the equation is:
\[ x + 3(+1) + (-2) + (+1) = 0 \]
\[ x + 3 - 2 + 1 = 0 \]
\[ x + 2 = 0 \]
\[ x = -2 \]

So, the oxidation number for carbon in CH₃OH(g) is -2.

### Step 2: Determine the Change in Oxidation Number
- In CO, carbon has an oxidation number of +2.
- In CH₃OH, carbon has an oxidation number of -2.

The change in oxidation number for carbon is from +2 to -2, indicating a decrease in oxidation number. This implies that carbon is being reduced.

### Step 3: Identify the Agent
- Reduction is a gain of electrons.
- Hydrogen is providing the electrons for the reduction of carbon.
- Therefore, hydrogen gas acts as the reducing agent.

### Step 4: Total Number of Electrons Transferred
- The oxidation number of carbon decreases from +2 to -2, which is a change of 4 units.
- Since the reaction involves 1 molecule of CO and 2 molecules of H₂, the total number of electrons transferred is 4.

### Summary
1. In the reaction represented above, hydrogen gas acts as the reducing agent, and the oxidation number for carbon in CO(g) decreases.

The correct row is:
- **Row**: iii (reducing, decreases)

2. The total number of electrons transferred in the industrial production of methanol is 4.

If you have any questions or need further details, feel free to ask!

### Questions to Ask
1. How do you determine the oxidation number changes in a redox reaction?
2. What is the role of a reducing agent in a chemical reaction?
3. How can you identify the number of electrons transferred in a redox reaction?
4. Why is it important to understand oxidation numbers in industrial chemical processes?
5. How do you balance redox reactions in terms of oxidation and reduction half-reactions?

### Tip
In redox reactions, the substance that gets reduced (gain of electrons) decreases in oxidation number, while the substance that gets oxidized (loss of electrons) increases in oxidation number.

Explore the industrial production of methanol through catalytic hydrogenation of carbon monoxide. Learn about redox reactions, oxidation numbers, and the role of hydrogen as a reducing agent. Discover the total number of electrons transferred in this chemical process.

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