Exam 18: Electrochemistry

The initial concentrations of Ag⁺(aq)and Cu²⁺(aq)are both 1.0 M.What will happen to the cell voltage if 5.0 M AgNO₃ is added to the compartment containing the 1.0 M Ag⁺(aq)? The cell voltage will

What is the molarity of a potassium triiodide solution,KI₃(aq),if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K₂S₂O₃(aq)? The chemical equation for the reaction is: 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq).

Shown below is an electrochemical cell with anode a and cathode c.Both the anode and the cathode are inert electrodes.The liquid shown in compartment b of the cell is molten potassium chloride,KCl(l). -Determine the direction of electron flow and the direction of ion flow.

Write the overall cell reaction for the galvanic cell given below. Pt(s)∣ H₂(g)∣ H⁺(aq)∣∣ Cl₂(g)∣ Cl^-(aq)∣ Pt(s)

The initial concentrations of Ag⁺(aq)and Cu²⁺(aq)are both 1.0 M.What will happen to the cell voltage if Cu(NO₃)₂ is added to the compartment containing the 1.0 M Cu²⁺(aq)? The cell voltage will

-Based on the following information, Cl₂(g)+ 2 e^- → 2 Cl^-(aq)E° = 1.36 V Zn²⁺(aq)+ 2 e^- → 2 Zn(s)E° = -0.76 V Which of the following chemical species is the strongest reducing agent?

A fuel cell is a galvanic cell in which the reactant is a fuel such as

A galvanic cell consists of a Al³⁺/Al half-cell and a standard hydrogen electrode.If the Al³⁺/Al half-cell standard cell functions as the anode,and the standard cell potential is 1.66 V,what is the standard reduction potential for the Al³⁺/Al half-cell?

Which of the following reactions is most suitable for a fuel cell?

In the galvanic cell represented by the shorthand notation below,electrons are lost by ________ and gained by ________. Pt(s)|Sn²⁺(aq)|Sn⁴⁺(aq)|| Br₂(l)|Br^-(aq)|Pt(s)

Based on the half-reactions and their respective standard reduction potentials below,the strongest reducing agent is ________,and the strongest oxidizing agent is ________. Ag⁺(aq)+ e^- → Ag(s)0.80 V 2 H⁺(aq)+ 2 e^- → H₂(g)0.00 V Pb²⁺(aq)+ 2 e^- → Pb(s)-0.13 V

Which requires the most electricity (in terms of faradays of charge transferred)per gram of useful product formed?

Shown below is a galvanic cell with anode compartment b containing anode a and cathode compartment d containing cathode c.Electrons flow through wire f,ions flow through salt bridge e,and the cell potential is read using voltmeter g. This galvanic cell uses the reaction: -Identify and give the sign of each electrode.

During an electrochemical reaction,electrons move through the external circuit toward the ________ and positive ions in the cell move toward the ________.

If the cell reaction involves ions in solution,as the cell reaction in a galvanic cell continues,

What are the coefficients in front of NO₃^-(aq)and Cu(s)when the following redox equation is balanced in an acidic solution: ________ NO₃^-(aq)+ ________ Cu(s)→ ________ NO(g)+ ________ Cu²⁺(aq)?

Based on the balanced chemical equation shown below,determine the molarity of a solution containing Fe²⁺(aq),if 40.00 mL of the Fe²⁺(aq)solution is required to completely react with 30.00 mL of a 0.500 M potassium bromate,KBrO₃(aq),solution.The chemical equation for the reaction is: 6 Fe²⁺(aq)+ BrO₃^-(aq)+ 6 H⁺(aq)→ 6 Fe³⁺(aq)+ Br^-(aq)+ 3 H₂O(l).

Redox reactions occurring in acid are evident by the appearance of ________ in the balanced equation,and redox reactions occurring in base are evident by the appearance of ________ in the balanced equation.

The equilibrium constant,K,can be calculated from

What are the coefficients in front of NO₃^-(aq)and Zn(s)when the following equation is balanced in a basic solution? ________ NO₃^-(aq)+ ________ Ni(s)→ ________ Ni²⁺(aq)+ ________ NO(g)