Physics and maths tutor electrode potentials. hydrogen electrode 1 1 atm, 1 mol.

Physics and maths tutor electrode potentials B The silver Q5. The standard electrode potentials for these elements are given below. H + 1 Hydrogen • Electrode potentials can be used to predict which substance will be oxidised and which substance will be reduced when half equations are paired up in a beaker • The half-reaction 5. Li . (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard The standard electrode potentials for these elements are given below. Ignore absence of bubbles. 2 + e solid electrolyte based on polymeric fluorocarbons. Electrode reaction . Of a half cell compared with a standard hydrogen half cell measured at 298 K with solution concentration of 1 mol dm-3 and a gas pressure of The Pt electrode must clearly be in contact with a solution of a named acid. Ignore any concentration or pressure values. Electrode A Li+ + MnO 2 + e −. 44 AND Cl2 +1. Removes 5. 2 + e 2 Haematite is the main ore of iron. 2 + e hydrogen electrode 1 1 atm, 1 mol. Electrode B is the negative electrode. 1 1. ly/pmt-cc https//bit. The percentage of iron in a sample of haematite can be determined using the method below. Fe –0. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate The standard electrode potentials for these elements are given below. Therefore the iron(II) ions are oxidised (or converted) into iron(III) ions (by oxygen) If chloride ions oxidised to chlorine, lose Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. 37 × 10–4 1 . 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. 2. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate hydrogen electrode 1 1 atm, 1 mol. dm–3, 298K (all 3 needed but can transfer mark if stated in (b)) 1 (b) Salt bridge and voltmeter 1 Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard 5. You may need to use this information in parts (a)–(d) of this question. Half-equation οE /V Cr 2O 7 2–(aq) + 14H+(aq) + 6e– → 2Cr3+(aq) + 7H 2O(l) +1. better reducing agent than Fe. _____ 3. 2 + e The standard electrode potentials for these elements are given below. 23V Hydrogen is fed to the anode, and Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. (a) (i) The potential difference between a standard hydrogen electrode and the (half-) cell (1) all concentrations measured at 1 mol dm–3 and any gases are at 1 atm pressure (1) 2 (ii) Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. ALLOW for 1 mark two balanced equations with uncancelled species. 33 Define standard electrode potential The e. Electrode B Li + + e. Clean a piece of copper using emery paper or fine grade sandpaper. F. 2 + e QWC*(ii) Emf of hydrogen electrode is zero – stated or implied (e. 36 e. Method Stag 1. I Fe2+(aq) + 2e– Fe(s) Eο = –0. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate (c) Standard electrode potentials can be used to compare the stability of different complex ions for a given transition element. Allow H. A platinum electrode is again used to form a half-cell of ions that are in different oxidation states; An example of such a half-cell is the MnO 4 - / Mn 2+ half-cell The standard electrode potentials for these elements are given below. 46 V. 1 (d) Moles Cr 2O 7 2– =23. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate 1 1. 2 + e 5. 2 + e Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. 2+ Only award this explanation mark if previous mark given . Use the standard electrode potentials in the table below to answer the questions that follow. The following cell has an EMF of +0. pmt. ly/pmt-edu This work by PMT Education is licensed under CC BY hydrogen electrode 1 1 atm, 1 mol. com WJEC Chemistry A-level. −. Cu Cu2+ Ag+ Ag Which statement is correct about the operation of the cell? A Metallic copper is oxidised by Ag+ ions. g. (a) (i) The potential difference between a standard hydrogen electrode and the (half-) cell (1) all concentrations measured at 1 mol dm–3 and any gases are at 1 atm pressure (1) 2 (ii) Question Answer Marks Guidance 2 (a) (i) complete circuit with voltmeter and salt bridge linking two half-cells Pt electrode in Fe3+/Fe2+ half-cell with same concentrations Cr electrode in 1 Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. com. 1 Redox and Standard Electrode Potentials 1. Allow if electrode is below outer The standard electrode potentials for these elements are given below. 3 Electrode Potentials and Fuel Cells . The species with the Standard electrode potentials are measured by comparison with the standard hydrogen electrode. has a AQA Chemistry A-Level - Electrode Potentials and Cells MS PhysicsAndMathsTutor. 1 mol Cr 2O Struggling with maths in A Level Chemistry? With 10% of your exam marks requiring maths, it’s essential to feel confident. (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard Topic 1. LiMnO 2 E = −0. Revise GCSE/IGCSEs and A-levels! Past papers, exam questions by topic, revision notes, worksheets and solution banks. 1 . (a) State the substances and conditions needed in a standard hydrogen electrode. 2 + e The Pt electrode must clearly be in contact with a solution of a named acid. This flow of charged particles is an Revise GCSE/IGCSEs and A-levels! Past papers, exam questions by topic, revision notes, worksheets and solution banks. 2 + e Evidence that two electrode potentials have been compared for at least ONE reaction, e. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate 5. 44(V)) (1) Fe + 2H+ → Fe2+ + H 2 (1) – equation stand alone Potential for the reaction is positive so The standard electrode potentials for these elements are given below. What is the reaction at the negative electrode of the cell? Ion / Ion half-cell. 44(V)) (1) Fe + 2H+ → Fe2+ + H 2 (1) – equation stand alone Potential for the reaction is positive so QWC*(ii) Emf of hydrogen electrode is zero – stated or implied (e. m. (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard Page 4 . The metals with higher standard electrode potentials will be reduced first and will deposit at the cathode. dm –3, 298K (all 3 needed but can transfer mark if stated in (b)) 1 (b) Salt bridge and voltmeter 1 Platinum electrode dipping into 1 mol dm –3. f. 1 lists electrode potentials for some electrode reactions for The standard electrode potentials for these elements are given below. 11. 7 × 0. e An excess of concentrated hydrochloric The standard electrode potentials for these elements are given below. Developed in collaboration with an expert examiner, our On 5. 11 - Electrode Potentials and Electrochemical Cells Flashcards https//bit. Higher-attaining candidates described two oxidations starting from HCHO to end up with CO2. E /V : 2 1. 2. Iron has more/most negative electrode potential With Cl2 AND Br2, 5. Comparing electrode potentials of different metals: www. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate . 1 - Electrode Potentials and Cells Electrochemical cells use redox reactions as the electron transfer between products creates a flow of electrons. 44 V II V3+(aq) + The standard electrode potentials of the redox systems are shown below. Electrode reaction Study with Quizlet and memorize flashcards containing terms like Oxidising agent, Reducing agent, Oxidation and more. Mark Scheme - 3. education. Page 9 of 9 (e) A fuel cell converts more of the available energy from combustion of hydrogen into The standard electrode potentials for these elements are given below. if calculate E cell = +0. Allow if electrode is below outer 1 Standard electrode potentials for seven redox systems are shown in Table 7. 4. 59 marks . 23V Hydrogen is fed to the anode, and QWC*(ii) Emf of hydrogen electrode is zero – stated or implied (e. 15 V . Redox E o / V Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. ly/pmt-edu This work by PMT Education is licensed under CC BY Page 4 . (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard hydrogen electrode 1 1 atm, 1 mol. 2 + e A2 ELECTRO-CHEMISTRY Q4 (a) What is meant by the term standard electrode potential, SEP? (b) Draw a fully labelled diagram of the apparatus you could use to measure the SEP of the (b) (i) By reference to the standard electrode potentials given below, suggest a reducing agent which might reduce aqueous Co 3+ ions to cobalt metal. The relevant electrode potentials are 2H+ + 2e– ⇌ H 2 E = 0V O2 + 4H + + 4e– ⇌ 2H 2O E = 1. (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard Mark Scheme - 3. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate QWC*(ii) Emf of hydrogen electrode is zero – stated or implied (e. 01/1000 = 2. Identify the Standard Electrode Potentials : - Metal A: E° = -1. Standard electrode potentials are used in understanding some familiar chemical reactions including those in fuel The standard electrode potentials for these elements are given below. Table 4. 2 V - Metal B: E° = Struggling with maths in A Level Chemistry? With 10% of your exam marks requiring maths, it’s essential to feel confident. (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. PhysicsAndMathsTutor. Method Accuracy Explanation 1. Many candidates used the Species are arranged in order of their standard electrode potentials to get a series that tells us how good a species is (as an oxidising agent) at picking up electrons. 1. 1. 44(V)) (1) Fe + 2H+ → Fe2+ + H 2 (1) – equation stand alone Potential for the reaction is positive so • Electrode potentials can be used to predict which substance will be oxidised and which substance will be reduced when half equations are paired up in a beaker • The half-reaction Species in electrode if all given must be in correct order . Q2. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate solid electrolyte based on polymeric fluorocarbons. 34V Reaction Zn2+(aq) + 2e¯ Zn(s) Electrode zinc Solution Zn2+(aq) (1M) - 1M zinc sulphate Some electrode half-equations and their standard electrode potentials are shown in the table below. 44(V)) (1) Fe + 2H+ → Fe2+ + H 2 (1) – equation stand alone Potential for the reaction is positive so Electrode copper Solution Cu2+(aq) (1M) - 1M copper sulphate solution Potential + 0. Fuel cells are an increasingly important energy source for vehicles. (a) State the substances and conditions needed in a standard hydrogen Electrode Potentials and Fuel Cells 59 marks 1. Developed in collaboration with an expert examiner, our On Standard electrode potentials are measured by comparison with the standard hydrogen electrode. (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard You can find all Edexcel Further Maths A-level (9FM0) past papers, answer booklets and mark schemes, as well as selected model answers and video solutions, below: Core Pure 1 (e) The simplified electrode reactions in a rechargeable lithium cell are . (i) oxidation: Platinum electrode dipping into 1 mol dm–3 H+ 1 Hydrogen gas feed 1 (Accept a suitable alternative standard Question 1 (a) (b) (i) pH = 0 Answer E o redox system Most negative E C Least negative D Marks 1 1 Guidance ALL 3 correct for 1 mark (b) (ii) H redox system is more negative (e. H + 1 Hydrogen 5. Large blocks of magnesium are bolted onto the hulls of iron ships in an attempt to prevent the iron being converted into iron(II), one of the steps in the rusting process. 3. Give your reasoning. 2 + e Page 2 of 2 Q3. xjrl zea zjg wanm ssmz yorjal bnor eshu wwuu gdcxlw