2CH3OH+3O2------> 2Co2 + 3H2O
carbon oxidation number increases from -2 to +4 . total 12 electrons are involve
G0 = -nE0 *F
-937900 =-12*E0 *96500
-937900 = -E0 *1158000
E0 = 937900/1158000 = 0.81V
The oxidation of methanol, as described by the equation below, has a deltaGdegree value of-937.9 kJ/mol....
M12. Methanol, CH3OH, has been considered as a possible fuel. Consider its oxidation: 2 CH3OH(1) + 3 O2(g) → 2 CO2(g) + 4H2O(g) AGºrx = -1372 kJ/mol What is the maximum work that can be obtained by oxidizing 0.50 mol of methanol under standard conditions?
The cell described by the net reaction. 2U(tl) + 3Cl_3(g) rightarrow 6Cl(aq) + 2U^+ (aq) has a standard deviation cell potential of + 3.16 V. The standard reduction potential for chlorine is: Cl_2(g) + 2e rightarrow 2Cl(aq) E degree = + 1.36 V What is the standard deduction potential of the U^3+(aq) | U(s) half-cell? A) -180 V B) + 1.80 V C) - 1.96 V D) -4.52 V E) +452 V Using the bond energies given below. estimate the...
could you please explain the problem with answers and explanations please ? (a) Write cathode and anode half-reactions, and a net reaction (balanced) for a low-temperature direct methanol fuel cell (assuming complete oxidation of fuel). Calculate the theoretical thermodynamic potential difference for an ideal direct methanol fuel cell (assuming complete oxidation of fuel) at 25.0 and 185 °C (F= 96485.3 Cmol-'). Standard thermodynamic data: AH:200) = -286 kJmol. Shop = 70.0 JK 'mol A.Hco2 = -394 kJmol. Sco2 = 214...
Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.08 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant Hg2+/Hg +0.85 F = 96485 C Fe3+/Fe2+ +0.77 2Fe3+(aq) + Hg(l) → 2Fe2+(aq) + Hg2+(aq) 2. The voltaic cell described by the balanced chemical equation has a standard emf of...
Methanol, CH3OH (l), combusts according to the following equation: 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l) ∆rHo (298 K) = −1452 kJ Here is a list of Entropies of formation: S (J K-1 mol-1) at 298 K CH3OH (l) =126.8 O2 (g) = 205.14 CO2 (g) = 213.74 H2O = (l) 69.91 (a) If the above reaction was used in a fuel cell, say, to perform work, what will be the maximum...
20. rBr 10,Br (in hasic solution) Final equation: 21 Predict the boiling point (in K) of cyclohexane using this data. (clearly show your work) Cyclohexane at its boiling point is described by the reactionCH..8 CHER-123 kJ/mol +298 J/mol-K Answer the next 5 questions with the following information: A voltaic cell is made with the metals Pb & Ag and the solutions Pb(NO)h& AgNO, at standard conditions 22. Write the half-steps for Oxidation: Reduction: 23. Write the balanced net ionic reaction:...
29. A process has a AHⓇ of 8.5 kJ/mol and a AS of 35.2 J/mol-K. What is AG at 300 K for this process? A) -23.0 kJ/mol B) -2.06 kJ/mol C) +33.4 kJ/mol D) +1.24 kJ/mol Sn (aq) 30. A spontaneous voltaic cell is based on the following two standard half-reactions: ca" () + 2e Cd () Eº rod (Cd?/Cd) = -0.40 V + 2e → Sn (1) E® red (Sn 2/Sn) = -0.14 V What is the standard cell...
29. A process has a AH° of 8.5 kJ/mol and a AS™ of 35.2 J/mol-K. What is AGº at 300 K for this process? A) -23.0 kJ/mol B) -2.06 kJ/mol C) +33.4 kJ/mol D) +1.24 kJ/mol cd2 (aq) + 2e Sn2 30. A spontaneous voltaic cell is based on the following two standard half-reactions: (aq) + 2e Cd (w) Eº red (Ca/Cd) = -0.40 V → Sn) Ered (Sn/Sn) = -0.14 V What is the standard cell potential, Ecell? A)...
Methanol (CH3OH) is used as a fuel in race cars. Part A Write a balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product. Express your answer as a chemical equation. Identify all of the phases in your answer. SubmitPrevious AnswersRequest Answer Incorrect; Try Again; 5 attempts remaining Part B Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product. Express your answer using four significant...
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...