If 0.30 mol of zinc are added to 0.52 mol of HCl, the moles of `H_(2)` formed are

Options

A. `0.52`
B. `0.30`
C. `0.26`
D. `0.60`

Explanation

To determine the moles of hydrogen gas (H₂) formed when 0.30 moles of zinc (Zn) are added to 0.52 moles of hydrochloric acid (HCl), we need to follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between zinc and hydrochloric acid can be represented by the following balanced equation:

\[ \text{Zn} + 2 \text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \]

### Step 2: Identify the mole ratio
From the balanced equation, we can see that:
- 1 mole of Zn reacts with 2 moles of HCl to produce 1 mole of H₂.

### Step 3: Determine the limiting reagent
We have:
- 0.30 moles of Zn
- 0.52 moles of HCl

To find the limiting reagent, we need to compare the amount of HCl required for the available Zn.

For 0.30 moles of Zn, the amount of HCl required is:
\[ 0.30 \text{ moles Zn} \times \frac{2 \text{ moles HCl}}{1 \text{ mole Zn}} = 0.60 \text{ moles HCl} \]

Since we only have 0.52 moles of HCl, HCl is the limiting reagent.

### Step 4: Calculate the moles of H₂ produced
Since HCl is the limiting reagent, we will use its amount to calculate the moles of H₂ produced.

From the balanced equation, 2 moles of HCl produce 1 mole of H₂. Therefore, the moles of H₂ produced from 0.52 moles of HCl is calculated as follows:

\[ 0.52 \text{ moles HCl} \times \frac{1 \text{ mole H}_2}{2 \text{ moles HCl}} = 0.26 \text{ moles H}_2 \]

### Conclusion
Thus, the moles of H₂ formed are **0.26 moles**.

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