Write the cell diagram for the following cell. KCl(aq) Zn Hg2Cl2(S) Pt Hg(1) ZnCl2(aq)
Consider the electrochemical cell: Pt(s)|Hg(l)| Hg2Cl2(s)|HCl(aq, 1.0M)|Hg(g,1 bar)|Pt(s) a.) write the overall balanced redox reaction. What is the notation saying up above. Please explain very stuck. b.) dH* > 0 and dS*>0 for the reaction. Upon increasing the temperature, will the cell potential 1.) increase 2.) decrease 3.) stay the same 4.) There is insufficient information to say. Please explain b. I don't even understand the question!
Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl2(aq) → ZnCl2(aq)+Fe(s) Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? Explanation Check © 2020 McGraw-Hill Education. All...
Zinc reacts with hydrochloric acid according to the reaction equation Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g)Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g) How many milliliters of 2.00 M HCl(aq)2.00 M HCl(aq) are required to react with 8.55 g Zn(s)?
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
8) Balance the equation for the following reaction. Zn(s) + HCl(1) → ZnCl2(aq) + H2(g) -
Consider the following cell at 25°C. Pt | Hg(l) | Hg2Clz(s) | HCl(aq,0.500 mol kgr) | Cl2(g) | Pt (i) Write the appropriate reduction half-reactions for the system above.(4) (i) Write the Nemst equation for the cell reaction. (ii) Assuming that the Debye-Hückel Limiting Law holds at the given concentration, calculate the potential E for the cell. (iv) Calculate for the cell reaction.
Which is the correct line notation for the galvanic cell you constructed using a Pb2+ solution, a Pb electrode and a Saturated Calomel Electrode (SCE) as reference? Hg Ι Hg2Cl2(s) Ι KCl(sat) ΙΙ Pb2+(aq) Ι Pb Pb2+(aq) Ι Pb ΙΙ KCl(sat) Ι Hg Ι Hg2Cl2(s) Pb Ι Pb2+(aq) ΙΙ KCl(sat) Ι Hg2Cl2(s) Ι Hg Hg Ι Pb2+(aq) ΙΙ KCl(sat) Ι Hg2Cl2(s) Ι Pb Which is the correct full oxidation/reduction equation for the copper/SCE galvanic cell that you investigated in Part C...
Determine S°rxn for Zn (s) + 2HCl (aq) ZnCl2 (aq) + H2 (g). Substance S° (J/mol ⋅ K) Zn(s) 60.9 HCl(aq) 56.5 H2(g) 130.58 Zn2+(aq) −106.5 Cl−(aq) 55.10 We were unable to transcribe this imageWe were unable to transcribe this image
In the following equation, what is oxidized? Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g) Group of answer choices Zinc Hydrogen in HCl Chlorine in HCl This is not an oxidation-reduction reaction
For the following electrochemical cell: Fe(s)| Fe3+(aq) || Cl(aq) | Cl2(g)|| Pt(s) a) Write the Cell Reaction for this Cell. b) Identify the Anode and Cathode.