Calculate E for the reduction of H+ to H2 at pH 2.0. (provide answer in V) |
Calculate E for the reduction of H+ to H2 at pH 2.0. (provide answer in V)
Calculate the reduction potential of the H+/H2 half reaction at 25 °C at pH 3.00 and PH2 = 0.20 bar. Assuming E° is unchanged, whatwould the potential be at 20 °C?
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° = 0.000 V E°cell (in V)= 0.126 V 2. The electrochemical cell is comprised of a Pb electrode in a 1.67 × 100 M solution of Pb2+ (aq) coupled to a Pt electrode in a solution containing H+ (aq) where the pH of the solution is 0.37 and the partial pressure of H2(g) is 0.571 atm. The temperature of the cell is held constant at...
Given that E o = 0.52 V for the reduction Cu+(aq) + e− → Cu(s), calculate E o , ΔG o , and K for the following reaction at 25°C: 2Cu+(aq) ⇌ Cu2+(aq) + Cu(s) E o = V ΔG o = kJ K = × 10 Enter your answer in scientific notation.
at The E, of the 2H+ + 2 e- → H2 half reaction is arbitrarily set at zero. Calculate E', pH 8. +0,378 V A. -0.286 V B. 0.143 V c .143 D. -0.143 V -0.472 v DE. 1 points Save Answer
44. Draw the reduction product of the below compound. Pt H2 H2 + H2 H3C Screen Shot 2020-07-30 at 11.59.55 AM Q Search v @ 50. Write the IUPAC name including cis or trans, if needed) for the following compound. (5 marks) H H3C H H2C-CH3
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.136 M), mixed with its conjugate base, A-(0.142 M). The measured cell voltage is E°cell = 0.196 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = _______ Ka = _______
18) Calculate the pressure of N2 if the equilibrium pressures of H2 = 2.0 atm, and NH3 = 0.5 atm, and Kp = 2.0 N2(g) + 3 H2(g) = 2 NH3(g) A) 0.031 atm (B).016 atm C) 0.062 atm D) 62,5 atm E) 0.40 atm 19) Consider the following reaction: CH4(g) + 2 H2S(g) = CS2(g) + 4 H2(g)
Part A Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.640 V when [Zn240.27 M and PH = 0.85 atm. Express your answer using two decimal places. V ΑΣφ pH =$ Figure 1 of 1 Previous Answers Request Answer Submit Switch 8.76 X Incorrect; Try Again; 2 attempts remaining Voltmeter Zn anode NO Na - H2(g) Cathode compartment (standard hydrogen electrode) NO3 Zn2 Provide Feedback Next Anode compartment NO3...
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...