The mass of silver in 9.000 g of silver chloride, AgCl(s), is:

Question

BlackTom AI · Accepted Answer

To determine the mass of silver in a given mass of silver chloride, we first need the proportion of silver in AgCl by mass.

Optionally, recall the molar masses: Ag ≈ 107.868 g/mol and Cl ≈ 35.453 g/mol, so the molar mass of AgCl is about 107.868 + 35.453 = 143.321 g/mol (rounded values may vary slightly, e.g., 143.315 g/mol in some tables).

Next, calculate the mass fraction of silver in AgCl: 107.868 / 143.315 ≈ 0.7526. This means about 75.26% of the mass of AgCl comes from silver.

Apply this fraction to the given mass of AgCl: 9.000 g × 0.7526 ≈ 6.773 g of Ag.

Now evaluate each answer choice:
- 7.527 g: This would correspond to a silver fraction of about 7.527 / 9.000 ≈ 0.836; this is too high and inconsistent with the actual composition of AgCl. It likely misuses the mass ratio or molar masses.
- 2.226 g: This would imply a silver fraction of about 2.226 / 9.000 ≈ 0.247; far smaller than the true 0.7526, indicating a misunderstanding of the compound’s composition.
- 6.280 g: This is somewhat close to 6.773 g but still noticeably low; it might result from using rounded molar masses or a rough fraction, but it does not match the precise calculation.
- 6.772 g: This value matches the calculated mass of Ag in 9.000 g of AgCl to three decimals, given the 0.7526 fraction. It aligns with standard stoichiometry.
- 8.343 g: This would require an even larger silver fraction (~0.926), which is inconsistent with AgCl’s composition and is therefore incorrect.

In summary, the correct approach uses the mass proportion of silver in silver chloride and applies it to the given mass, yielding approximately 6.773 g of Ag, which corresponds to the option 6.772 g (within typical rounding).

The mass of silver in 9.000 g of silver chloride, AgCl(s), is:

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