What mass of `CH_(3)OH ("methanol")` will be produced by reacting `1120L` of `H_(2)(g)` at `STP` with excess `CO(g)` ? .

Explanation

To find the mass of methanol (CH₃OH) produced from the reaction of hydrogen gas (H₂) with excess carbon monoxide (CO), we will follow these steps:

### Step 1: Write the balanced chemical equation
The balanced equation for the reaction is:
\[ \text{CO (g)} + 2 \text{H}_2 (g) \rightarrow \text{CH}_3\text{OH (l)} \]

### Step 2: Calculate the moles of H₂
At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 liters. We need to calculate the number of moles of hydrogen gas (H₂) in 1120 liters.
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