A sample of pure CuO was reduced with `H_2` gas and `H_(2)O` formed was collected in a 44.8 L flask containing dry `N_(2)`. At `27^@C`, the total pressure containing `N_(2)` and `H_(2)O` was 1.0 atm. Relative humidity in the flask was `80%` The vapour pressure of water at `27^@C` is 25 mm. How many grams of CuO was reduced?

Explanation

To solve the problem step by step, we will follow these instructions:

### Step 1: Write the reaction
The reduction of copper(II) oxide (CuO) with hydrogen (H₂) can be represented by the balanced chemical equation:
\[ \text{CuO} + \text{H}_2 \rightarrow \text{Cu} + \text{H}_2\text{O} \]

### Step 2: Convert the total pressure to mmHg
Given that the total pressure is 1.0 atm, we can convert this to mmHg:
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