Which of the following has the highest mass?

Options

A. 1 g - atom of C
B. `(1)/(2)"mole of" CH_(4)`
C. 10ml of water
D. `3.011xx10^(23)` atoms of oxygen

Explanation

To determine which of the given options has the highest mass, we will analyze each option step by step.

### Step 1: Analyze Option A
- **Option A**: 1 gram atom of carbon.
- The atomic mass of carbon (C) is approximately 12 grams/mole.
- Therefore, 1 gram atom of carbon is equal to 12 grams.

### Step 2: Analyze Option B
- **Option B**: 1/2 mole of methane (CH₄).
- The molar mass of methane (CH₄) is calculated as follows:
- Carbon (C) = 12 g/mol
- Hydrogen (H) = 1 g/mol × 4 = 4 g/mol
- Total = 12 g/mol + 4 g/mol = 16 g/mol
- Therefore, 1/2 mole of CH₄ = 16 g/mol × 0.5 = 8 grams.

### Step 3: Analyze Option C
- **Option C**: 10 ml of water.
- The density of water is 1 g/ml.
- Therefore, 10 ml of water = 10 ml × 1 g/ml = 10 grams.

### Step 4: Analyze Option D
- **Option D**: 3.011 × 10²³ atoms of O₂.
- The molar mass of O₂ is approximately 32 grams/mole.
- 1 mole of O₂ contains 6.022 × 10²³ molecules (Avogadro's number).
- To find the mass of 3.011 × 10²³ atoms of O₂:
- Calculate the number of moles:
\[ \text{Number of moles} = \frac{3.011 \times 10^{23}}{6.022 \times 10^{23}} = 0.5 \text{ moles} \]
- Therefore, the mass of 0.5 moles of O₂ = 0.5 moles × 32 g/mole = 16 grams.

### Step 5: Compare All Options
- Option A: 12 grams
- Option B: 8 grams
- Option C: 10 grams
- Option D: 16 grams

### Conclusion
The highest mass among the options is from **Option D**, which is 16 grams.

### Final Answer
**Option D has the highest mass.**

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