63. A sample of unknown metal is placed in a graduated cylinder containing water. The mass of the sample is 37.5 g, and the water levels before and after adding the sample to the cylinder are as shown in the figure. Which metal in the following list is most likely the sample? (d is the density of the metal.) Vi = 7 ml and Vf = 20.5 ml (a) Mg, d = 1.74 g/cm3 (b) Fe, d = 7.87 g/cm3 (c) (c) Ag, d = 10.5 g/cm3 (d) Al, d = 2.70 g/cm3 (e) Cu, d = 8.96 g/cm3 (f) Pb, d = 11.3 g/cm3

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Chapter1: Chemical Foundations
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**Question 63:**

A sample of unknown metal is placed in a graduated cylinder containing water. The mass of the sample is 37.5 g, and the water levels before and after adding the sample to the cylinder are shown in the figure. Which metal in the following list is most likely the sample? (d is the density of the metal.)

- Initial volume (Vi) = 7 ml
- Final volume (Vf) = 20.5 ml

**Options:**

(a) Mg, \(d = 1.74 \, \text{g/cm}^3\)

(b) Fe, \(d = 7.87 \, \text{g/cm}^3\)

(c) Ag, \(d = 10.5 \, \text{g/cm}^3\)

(d) Al, \(d = 2.70 \, \text{g/cm}^3\)

(e) Cu, \(d = 8.96 \, \text{g/cm}^3\)

(f) Pb, \(d = 11.3 \, \text{g/cm}^3\)

**Explanation:** 

The volume of the metal sample is found by the displacement of water, calculated as follows:
\[ \text{Volume of sample} = Vf - Vi = 20.5 \, \text{ml} - 7 \, \text{ml} = 13.5 \, \text{ml} \]

Using the formula for density, \(\text{Density} = \frac{\text{Mass}}{\text{Volume}}\), the density of the sample can be calculated:
\[ \text{Density} = \frac{37.5 \, \text{g}}{13.5 \, \text{ml}} = 2.78 \, \text{g/cm}^3 \]

Matching this calculated density with the options provided, the metal is most likely Aluminum (Al) with \(d = 2.70 \, \text{g/cm}^3\).
Transcribed Image Text:**Question 63:** A sample of unknown metal is placed in a graduated cylinder containing water. The mass of the sample is 37.5 g, and the water levels before and after adding the sample to the cylinder are shown in the figure. Which metal in the following list is most likely the sample? (d is the density of the metal.) - Initial volume (Vi) = 7 ml - Final volume (Vf) = 20.5 ml **Options:** (a) Mg, \(d = 1.74 \, \text{g/cm}^3\) (b) Fe, \(d = 7.87 \, \text{g/cm}^3\) (c) Ag, \(d = 10.5 \, \text{g/cm}^3\) (d) Al, \(d = 2.70 \, \text{g/cm}^3\) (e) Cu, \(d = 8.96 \, \text{g/cm}^3\) (f) Pb, \(d = 11.3 \, \text{g/cm}^3\) **Explanation:** The volume of the metal sample is found by the displacement of water, calculated as follows: \[ \text{Volume of sample} = Vf - Vi = 20.5 \, \text{ml} - 7 \, \text{ml} = 13.5 \, \text{ml} \] Using the formula for density, \(\text{Density} = \frac{\text{Mass}}{\text{Volume}}\), the density of the sample can be calculated: \[ \text{Density} = \frac{37.5 \, \text{g}}{13.5 \, \text{ml}} = 2.78 \, \text{g/cm}^3 \] Matching this calculated density with the options provided, the metal is most likely Aluminum (Al) with \(d = 2.70 \, \text{g/cm}^3\).
**Equilibrium Reactions in Aqueous Solutions of Acids**

**15.** Equal amounts of two acids—HCl and HCO₂H (formic acid)—are placed in aqueous solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the HCO₂H solution. Which reaction is more product-favored at equilibrium?

**Reactions:**
- HCl(aq) + H₂O(ℓ) ⇌ H₃O⁺(aq) + Cl⁻(aq)
- HCO₂H(aq) + H₂O(ℓ) ⇌ H₃O⁺(aq) + HCO₂⁻(aq)

**Explanation:**

In the context of these two reactions, the electrical conductivity of the solution serves as an indicator of the concentration of ions in the solution. The greater electrical conductivity observed in the HCl solution suggests that the dissociation of HCl in water to form hydronium ions (H₃O⁺) and chloride ions (Cl⁻) is more complete, thus favoring the products. This indicates that the reaction of HCl is more product-favored compared to the dissociation of formic acid (HCO₂H) under similar conditions.
Transcribed Image Text:**Equilibrium Reactions in Aqueous Solutions of Acids** **15.** Equal amounts of two acids—HCl and HCO₂H (formic acid)—are placed in aqueous solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the HCO₂H solution. Which reaction is more product-favored at equilibrium? **Reactions:** - HCl(aq) + H₂O(ℓ) ⇌ H₃O⁺(aq) + Cl⁻(aq) - HCO₂H(aq) + H₂O(ℓ) ⇌ H₃O⁺(aq) + HCO₂⁻(aq) **Explanation:** In the context of these two reactions, the electrical conductivity of the solution serves as an indicator of the concentration of ions in the solution. The greater electrical conductivity observed in the HCl solution suggests that the dissociation of HCl in water to form hydronium ions (H₃O⁺) and chloride ions (Cl⁻) is more complete, thus favoring the products. This indicates that the reaction of HCl is more product-favored compared to the dissociation of formic acid (HCO₂H) under similar conditions.
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