The standard cell potential for the fuel cell 2
H2(g) + O2(g)
⇔ 2 H2O(l) is
=
+1.23 V at 298 K and +1.18 at 358 K. Estimate the standard entropy
change of the cell reaction.
The standard cell potential for the fuel cell 2 H2(g) + O2(g) ⇔ 2 H2O(l) is = +1.23 V at 298 K and +1.18 at...
The standard cell potential for the fuel cell 2 H2(g) + O2(g) → 2 H2O(l) is E° = +1.23 V at 298 K and +1.18 at 358 K. Estimate the standard entropy change of the cell reaction. Use Table 7.1. to determine v (E-E) A. Sº = vF 7. 0 -160 J mol-1 K-1 0-320 J mol-1 k-1 O-107 J mol-1 K-1 0 -80 J mol-1 k-1
P6C.2 Calculate the value of A_G®(H,0,1) at 298 K from the standard potential of the cell Pt(s)[H2(g)|HCl(aq)|O2(g)|Pt(s), El = +1.23 V.
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),...
In a hydrogen fuel cell, oxygen and hydrogen are combincd to produce water and a small potential differ- ence. The steps of the chemical reaction are: at-electrode: at + electrode: H2 + 20H-→ 2H2O + 2e-; O2 + H2O + 2e-→ 2OH-, Use the table of chemical values to calculate a) the work that can be produced from this fuel cell, b) the 'waste' heat produced during standard operation, c) the voltage of the cell, and d) the minimum voltage...
The standard enthalpy change for the following reaction is - 52.3 kJ at 298 K. C2H4(g) — 2 C(s.graphite) + 2 H2(g) AH° = -52.3 kJ What is the standard enthalpy change for this reaction at 298 K? 2 C(s,graphite) + 2 H2(g) — C2H4(9) LLUCU The standard enthalpy change for the following reaction is -240 kJ at 298 K. Ni(s) + 1/2 O2(g) → Nio(s) AH° = -240 kJ What is the standard enthalpy change for the reaction at...
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205
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...
4. The reduction of O2 to H2O in aqueous acid is an important half-reaction in the operation of hydrogen-powered fuel cells, a type of galvanic cell. The standard reduction potential for this half-reaction is 1.23 V at 25°C. O2 (aq) + 4H+ (aq) + 40-42 H20 (1) If the pH at the cathode of a fuel cell were to be increased by one full unit, what would be the change (in millivolts) to this half-cell's potential? ||
The standard enthalpy change for the following reaction is -426 kJ at 298 K. Na(s) + 1/2 O2(g) + 1/2 H2(g) → NaOH(s) AH° = -426 kJ What is the standard enthalpy change for the reaction at 298 K? 2 Na(s) + O2(0)+ H2()—2 NaOH(s) The standard enthalpy change for the following reaction is 484 kJ at 298 K. CH3COOH(1) ► 2 C(s,graphite) + 2 H2(g) + O2(g) AH° = 484 kJ What is the standard enthalpy change for this...
The standard potential for the cell Cl2(g) + Cu(s) CuCl2(aq) is +1.02 V. Determine the potential of the cell at 298 K when the partial pressure of chlorine gas is 0.100 bar and the concentration of copper(II) chloride is 0.017 mol dm3 How many ions are in sol'n? +1.02 V O +1.13 V +1.23 V +0.91V