Silver chloride formula percent composition
a) AgCl, 75% Ag, 25% Cl
b) AgCl, 50% Ag, 50% Cl
c) AgCl, 60% Ag, 40% Cl
d) AgCl, 40% Ag, 60% Cl
The Correct Answer and Explanation is :
The correct percent composition of silver chloride (AgCl) is a) AgCl, 75% Ag, 25% Cl.
Explanation
To determine the percent composition of silver chloride, we first need to calculate the molar mass of AgCl. The molar mass is the sum of the atomic masses of its constituent elements: silver (Ag) and chlorine (Cl).
- Atomic mass of silver (Ag): approximately 107.87 g/mol
- Atomic mass of chlorine (Cl): approximately 35.45 g/mol
Calculating the molar mass of AgCl:
[
\text{Molar mass of AgCl} = \text{Atomic mass of Ag} + \text{Atomic mass of Cl}
]
[
= 107.87 \, \text{g/mol} + 35.45 \, \text{g/mol}
]
[
= 143.32 \, \text{g/mol}
]
Next, we calculate the percent composition of each element in AgCl using the formula:
[
\text{Percent composition} = \left( \frac{\text{mass of element}}{\text{molar mass of compound}} \right) \times 100
]
Percent composition of silver (Ag):
[
\text{Percent Ag} = \left( \frac{107.87}{143.32} \right) \times 100 \approx 75.24\%
]
Percent composition of chlorine (Cl):
[
\text{Percent Cl} = \left( \frac{35.45}{143.32} \right) \times 100 \approx 24.76\%
]
These calculations indicate that silver chloride is composed of approximately 75% silver and 25% chlorine by mass, matching the option a).
The other options do not correspond to the actual mass percentages derived from the molar masses. For example, option b) claims a 50% composition for both elements, which is incorrect based on the calculated molar mass. Similarly, options c) and d) provide inaccurate ratios that do not align with the fundamental chemistry of AgCl.
Thus, the accurate percent composition of silver chloride is approximately 75% Ag and 25% Cl, confirming option a) as the correct answer.