Based on the cell potentials in the previous question calculate equilibrium constant of the following reaction
H2(g) + I2 (g) → 2HI(aq)
Please enter your answer using E notation with 2 decimals. for example, 1234.456 is written as 1.23E3
Based on the cell potentials in the previous question calculate equilibrium constant of the following reaction...
Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction: Cu(s) +2Ag (aq)Cu2+ 2Ag(s) Report the answer in volts with three significant figures 0.442 Previous Answers Request Answer Submit X Incorrect; Try Again; 3 attempts remaining Review your calculations; you may have made a rounding error or used the wrong number of significant figures. Part B Determine the equilibrium constant for the above reaction Report to 1 significant figure and using scientific notation 9.1014
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I(aq) A.8.9 × 10-18 B.1.1 × 1017 C.1.7 × 1029 D.2.4 × 1058 E.3.5 × 10-59
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
Be sure to answer all parts. Use standard reduction potentials to find the equilibrium constant for the following reaction at 25 °C: Br2(aq) + 2I−(aq) ⇌ 2Br−(aq) + I2(s) Enter your answer in scientific notation to one significant digit. K = ___×___ 10
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe(a 2Fe(a) Fe(s)+2Fe (aq) Hint: Carry at least Equilibrium constant: than zero. AO for this reaction would be 9 more group a Submit Answer Retry Entire Group ing Use standard reduction potentials to calculate the equilibrium constant for the reaction: Sn2+(aq) + Fe(s)-→ Sn(s) + Fe2+(aq) Hint: Carry at least S significant figures during intermediate calculations to avoid round off error when taking the antilogarithnm. Equilibrium constant AG°...
question 1 -
Use standard reduction potentials to calculate the equilibrium
constant for the reaction:
Fe3+(aq) +
Cu+(aq)
Fe2+(aq) +
Cu2+(aq)
Carry at least 5 significant figures during intermediate
calculations to avoid roundoff error when taking the
antilogarithm.
Equilibrium constant: ..... ?
G° for this
reaction would be greater or less than zero.?
question 2
Use standard reduction potentials to calculate the equilibrium
constant for the reaction:
2Cu2+(aq)
+ Hg(l)2Cu+(aq)
+ Hg2+(aq)
Carry at least 5 significant figures during intermediate...
The equilibrium constant, Kc, for the following reaction is 2.02×10-2 at 745 K. 2HI(g) <--> H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) <--> 2HI(g) Kc =
The equilibrium constant, Kc, for the following reaction is 1.68×10-2 at 672 K. 2HI(g) <---> H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) <---> 2HI(g) Kc =
A. Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H+(aq) + Fe(s) H2(g) + Fe2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: _____ G° for this reaction would be _____ (greater/less) than zero. B. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd2+(aq) + 2Ag(s)Cd(s) + 2Ag+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to...
The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at698 K.2HI(g) → H2(g) + I2(g)Calculate the equilibrium concentrations of reactant and products when 0.223 moles of HI are introduced into a 1.00 L vessel at 698 K.[HI]= ?[H2]= ?[I2]= ?