Consider the following reagents: zinc, copper, mercury (density \(13.6 \mathrm{~g} / \mathrm{mL}\) ), silver nitrate solution, nitric acid solution. (a) Given a \(500-\mathrm{mL}\) Erlenmeyer flask and a balloon can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?

Step by step solution

01

(a) Chemical reaction that inflates the balloon

To inflate a balloon, a gas must be produced from the chemical reaction. A possible chemical reaction that involves given reagents that produces a gas is: Zinc (Zn) reacts with nitric acid (HNO₃) to produce hydrogen gas (H₂) as a byproduct. The balanced chemical equation for this reaction can be written as: \[ Zn + 2HNO_3 \rightarrow Zn(NO_3)_2 + H_2 \] The hydrogen gas (H₂) produced in this reaction will inflate the balloon.

02

(b) Theoretical yield of hydrogen gas

To calculate the theoretical yield of hydrogen gas, we need the mass of zinc and the concentration of nitric acid used in the reaction. Since the mass and concentration are not provided in the given exercise, we will generalize the method to calculate the theoretical yield given any mass and concentration. 1. Convert the mass of zinc (m_zn) to moles using the molar mass of zinc (M_zn = 65.38 g/mol): \[n_{Zn} = \frac{m_{Zn}}{M_{Zn}} \] 2. Use the stoichiometry of the balanced reaction to find the moles of hydrogen gas produced (n_H2): \[ n_{H_2} = \frac{1}{2} n_{Zn} \] 3. Convert the moles of hydrogen gas to grams using the molar mass of hydrogen (M_H2 = 2.01 g/mol): \[ m_{H_2} = n_{H_2} \times M_{H_2} \] The theoretical yield of hydrogen gas can be calculated by following those steps.

03

(c) Chemical reaction that produces metallic silver and ions left in solution

In order to produce metallic silver, we can dissolve copper (Cu) in silver nitrate (AgNO₃). The chemical equation for this reaction is: \[ Cu + 2AgNO_3 \rightarrow Cu(NO_3)_2 + 2Ag \] Metallic silver (Ag) is produced, while copper(II) nitrate (Cu(NO₃)₂) and nitrate (NO₃⁻) ions are left in the solution.

04

(d) Theoretical yield of metallic silver

To calculate the theoretical yield of metallic silver, we need the mass of copper and the concentration of silver nitrate used in the reaction. As the mass and concentration are not provided in the given exercise, we will generalize the method to calculate the theoretical yield given any mass and concentration. 1. Convert the mass of copper (m_Cu) to moles using the molar mass of copper (M_Cu = 63.55 g/mol): \[ n_{Cu} = \frac{m_{Cu}}{M_{Cu}} \] 2. Use the stoichiometry of the balanced reaction to find the moles of metallic silver produced (n_Ag): \[ n_{Ag} = 2n_{Cu} \] 3. Convert the moles of metallic silver to grams using the molar mass of silver (M_Ag = 107.87 g/mol): \[ m_{Ag} = n_{Ag} \times M_{Ag} \] The theoretical yield of metallic silver can be calculated by following those steps.

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