A cup contains 250 g of water. Find the total positive charge present in the cup of water.

Options

A. `1.34xx10^(19) C`
B. `1.34xx10^(7) C`
C. `2.43xx10^(19) C`
D. `2.43xx10^(7) C`

Explanation

To find the total positive charge present in a cup of water containing 250 g of water, we can follow these steps:

### Step 1: Convert the mass of water to grams
The mass of water is already given as 250 g.

### Step 2: Calculate the number of moles of water
The molecular mass of water (H₂O) is approximately 18 g/mol. To find the number of moles (n) of water, we use the formula:

\[ n = \frac{m}{M} \]

where:
- \( m \) = mass of water = 250 g
- \( M \) = molecular mass of water = 18 g/mol

Substituting the values:

\[ n = \frac{250 \, \text{g}}{18 \, \text{g/mol}} \approx 13.89 \, \text{mol} \]

### Step 3: Calculate the number of water molecules
Using Avogadro's number (\( N_A \)), which is approximately \( 6.02 \times 10^{23} \) molecules/mol, we can find the total number of water molecules:

\[ \text{Number of molecules} = n \times N_A \]

Substituting the values:

\[ \text{Number of molecules} = 13.89 \, \text{mol} \times 6.02 \times 10^{23} \, \text{molecules/mol} \approx 8.36 \times 10^{24} \, \text{molecules} \]

### Step 4: Calculate the total positive charge
Each water molecule (H₂O) contains 2 hydrogen atoms, each contributing a positive charge of \( +1.6 \times 10^{-19} \) C. Therefore, the total positive charge (Q) can be calculated as:

\[ Q = \text{Number of molecules} \times \text{Charge per hydrogen atom} \times 2 \]

Substituting the values:

\[ Q = 8.36 \times 10^{24} \, \text{molecules} \times 2 \times 1.6 \times 10^{-19} \, \text{C} \]

Calculating this gives:

\[ Q \approx 2.67 \times 10^{6} \, \text{C} \]

### Final Result
The total positive charge present in the cup of water is approximately \( 2.67 \times 10^{6} \, \text{C} \).

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