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Calculate the standard potential, ?∘, for this reaction from its equilibrium constant at 298 K.
Calculate the standard potential, Eº, for this reaction from its equilibrium constant at 298 K. X(s) + y2+(aq) = x2+(aq) + Y(s) K = 9.95 103 E = V
Calculate the standard potential, E®, for this reaction from its equilibrium constant at 298 K. X(s) +Y4+ (aq) = X4+ (aq) + Y(s) K = 7.92 x 10-8 E =
The equilibrium constant, Kp, for the following reaction is 0.160 at 298 K. Calculate K, for this reaction at this temperature. 2NOBr(g) 2NO(g) + Br2(g) Kc =
Calculate the equilibrium constant K at 298 K for the following reaction: 3C2H2 → C6H6 ?G f^o(C2H2) = 209.2 kJ/mol, ?G f^o(C6H6) = 129.7kJ/mol Choices: a.) 3.33*10^95 b.) 2.57*10^45 c.) 6.53 * 10^30 d.) 1.96*10^87
a.) Calculate the equilibrium constant for the following reaction at 298.15 K from cell potential data. Express the answer as lnK. Sn4+ + 2Fe2+ ----> Sn2+ + 2Fe3+ b.) Calculate the standard Gibbs free energy change in kJ/mol at 298.15 K for the following reaction from cell potential data: 3Sn4+ + 2Cr ----> 3Sn2+ + 2Cr3+
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation Fe(s) + Ni+ (aq) +Fe?+ (aq) + NI(s) FE In K = Express your answer numerically. View Available Hints) where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mole). R (the gas constant) is equal to 8.314 J/(mol-K). and T is the Kelvin temperature. ΟΙ ΑΣΦ h ? KK- Submit Previous Answers *...
The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by the equation lnK=nFE∘RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e−) , R (the gas constant) is equal to 8.314 J/(mol⋅K) , and T is the Kelvin temperature. Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 5.51×10−3.
At 298 K a cell reaction has a standard emf of +0.18 V. The equilibrium constant for the cell reaction is 5.6×105 What is the value of n for the cell reaction? Please explain this problem to me.
A reaction has an equilibrium constant of 8x103 at 298 K. At 716 K, the equilibrium constant is 0.77. Find AHºrxn for the reaction. Enter your answer numerically in kJ to 4 decimal places.