Calculate the mass in grams of 0.13 mole of `H_2S`.

Options

A. 4.42g
B. 5.48g
C. 3.48g
D. 2.45g

Explanation

To calculate the mass in grams of 0.13 moles of \( H_2S \), we can follow these steps:

### Step 1: Determine the Molar Mass of \( H_2S \)
- The molar mass of a compound is the sum of the atomic masses of all the atoms in the molecule.
- For \( H_2S \):
- Hydrogen (H) has an atomic mass of approximately 1 g/mol. Since there are 2 hydrogen atoms, the contribution from hydrogen is:
\[ 2 \times 1 = 2 \, \text{g/mol} \]
- Sulfur (S) has an atomic mass of approximately 32 g/mol. Therefore, the contribution from sulfur is:
\[ 32 \, \text{g/mol} \]
- Adding these together gives the molar mass of \( H_2S \):
\[ \text{Molar mass of } H_2S = 2 + 32 = 34 \, \text{g/mol} \]

### Step 2: Use the Molar Mass to Calculate the Mass
- We know that the number of moles (n) is related to mass (m) and molar mass (M) by the formula:
\[ n = \frac{m}{M} \]
- Rearranging this formula to find the mass gives:
\[ m = n \times M \]
- Substituting the values we have:
\[ m = 0.13 \, \text{moles} \times 34 \, \text{g/mol} \]

### Step 3: Perform the Calculation
- Now, we can calculate the mass:
\[ m = 0.13 \times 34 = 4.42 \, \text{grams} \]

### Final Answer
- The mass of 0.13 moles of \( H_2S \) is **4.42 grams**.

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