Part CConsider the following reaction:СО (9) + 2H2 (9) — СH3ОН (9)K, = 2.26 x 104 at 25 °C. Calculate AGrxn forthe reaction at 25 °C under each of the followingРСH,ОН 3 1.1 аtm;Pco = PH, = 1.5x10-2 atmconditions.Express your answer using two significantfigures.ΑΣφAGrxn - 31Submit

Answered: Image /qna-images/answer/301b4d93-d770-4e47-b25f-a377d90eadb4.jpg

Part C Consider the following reaction: CO (g) + 2H2 (g) K, = 2.26 x 104 at 25 °C. Calculate AGrxn for the reaction at 25 °C under each of the following = CH3OH (g) Рен,Он — 1.1 atm; Pco = PH, = 1.5x10-2 atm conditions. Express your answer using two significant figures. ΑΣφ AGrxn - 31 | II

Part C Consider the following reaction: CO (g) + 2H2 (g) K, = 2.26 x 104 at 25 °C. Calculate AGrxn for the reaction at 25 °C under each of the following = CH3OH (g) Рен,Он — 1.1 atm; Pco = PH, = 1.5x10-2 atm conditions. Express your answer using two significant figures. ΑΣφ AGrxn - 31 | II

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

See similar textbooks

Similar questions

Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
Assuming the equilibrium constants at 200°C for the following reactions are given below, NH4"(aq) + H20() NH3(ag) + H30*(aq); K1 = 6.48 x 10-7 CH3COOH(aq) + H2O(/). CH3COO (aq) + H30*(aq); K2 = 2.72x 10-5 determine Ke for the following equilibrium. CH3COOH(aq) + NH3(aq) CH3CO0 (aq) + NH4"*(aq) Please keep your answer to one decimal place.
Calculate AG and the exponent value (the x of 10) for K, for the following reactions at 25°C: (a) Mg(s) + Pb²*(aq) = Mg²"(aq) + Pb(s) AG :-430.3 x: 75 (b) O2(8) + 4H (aq) + 4FE2"(aq) 2H,O(!) + 4Fe* (aq) AG :-177.5 x: 31 (c) 2Al(s) + 312(s) 2A1*(aq) + 6T (aq) AG 1280.4 x:23
3.81944444 Be sure to answer all parts. The AG° for the reaction H;2) + I;(2) = 2HI(g) is 2.60 k.J'mol at 25°C. In one experiment, the initial pressures are PH, = 3.96 atm P, = 0.020 atm PHI = 0.55 atm Calculate AG for the reaction and predict the direction of the net reaction. kJimol The net reaction proceeds from left to right The reaction proceeds from right to left
The autoionization constant of water (K„) is 1.139 × 10-15 at 0°C and 9.614 × 10-14 at 60°C. (a) Calculate the standard enthalpy of autoionization of water. 2 H2O(€)2 H;O*(aq) + OH¯(aq) (b) Calculate the standard entropy of autoionization of water. (c) At what temperature will the pH of pure water be 7.00, from these data?
The bisulfate (or hydrogen sulfate) anion, HSO4 , is a weak acid. The equilibrium constant for the aqueous acid reaction HSO4 (ag) = H* (ag) + SO,2- (ag) is 1.2 x 10-2 (a) Calculate AG° for this equilibrium. Assume a tempera- ture of 25.0°C. (b) At low concentrations, activity coefficients are approxi- mately 1 and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a 0.010-molal solution of sodium hydrogen sulfate.
What is the pH of the saturated solution of iron(II) hydroxide at about 98° C: Fe(OH),(s) 2 Fe"(aq) + 20H (aq), Ksp = 5.0x10-13 Round off your answer to 3 sig. figs., and enter it in the box provided with correct units: The pH of the saturated Answer: solution of Fe(OH), is : pH =
The equilibrium constant of the reaction 2 C3H6 (g) ⇌ C2H4(g) + C4H8(g) is found to fit the expression InK= -1.04-(1088 K)/T +(1.51 x 10-2 K2)/T2between 300 K and 600 K. (a) Calculate the standard reaction Gibbs energy at each temperature at 390 K and 410 K. (b) Use the van 't Hoff equation to determine the standard reaction enthalpy at 400 K. (c) Hence also calculate the standard reaction entropy at 400 K.
J R = 8.314 mol·K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H"(aq) + 4 e 2 H20 (1) 1.229 |Z2 (s) + 2 e → 2Z° (aq) 0.426 3+ (aq) + 3 е A' → A (s) 0.292 2 H20 (I) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 G2+ (aq) + 2 e G (s) - 1.245 (aq) + 2 e¯ → M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 MMZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 11 The electrode connected to the red wire (negative terminal on the battery) will... o produce bubbles and the pH will increase. o produce M (s) on the electrode and the pH will not change. o produce bubbles and the pH will decrease. o produce M (s) on the electrode and the pH will decrease. Question 12 The electrode…
Given the dissociation reaction, Br2(g) = 2 Br(g), AH = + 112 kJ mol^ - 1 molecular bromine is 35 per cent dissociated at 1600 K and 1.00 bar at equilibrium. Calculate the equilibrium constant, K at 25\deg C. At what temperature would the reaction mixture need to be to turned off, ~ K = 10^-5?
Consider the reaction at 25 degrees celsius 2NO3-(aq)+8H+(aq)+3Cu(s)=3Cu2+(aq)+2NO(g)+4H2O(l) At what pH is the reaction at equilibrium with all other ionic species at 0.01M and gases at 1 atm?
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?