Corrosion of iron in water is given by, Fe° + 2H + Fe+2 + H2(g) Calculate equilibrium constant at 298 K. Calculate pH2 when pH = 10 and [Fe*] = 10-³ M. O Keq = 7.49x10^14; PH2 = 0.00749 atm %3D %3D Keq = 3.64x10^13; PH2 = 0.0036 atm %3D %3D Keq = 7.69×10^12; PH2 = 0.0065 atm %3D %3D Keq = 2.49x10^14; %3D PH2 = 0.0749 atm %3D Next

Nitrous acid, HNO2 , is a weak acid that ionizes according to the reaction HNO2 (aq) + H2O(l) ⇄ H3O+(aq) + NO-2 (aq) If the equilibrium constant, Kc, for the reaction above is 3.3x10-5 what is the H3O+ concentration for a 1M solution of nitrous acid?

I only need help with question C

How long, in minutes, will it take to produce 54.5 grams of Fe(l) if 80.4 Amps are passed through a solution of FeBr3?

its also not 4.57e-13

Topics: Cells and equilibrium; Competing equilibrium in cells Use general chemistry rules for significant figures. 1. Calculate the equilibrium constant for: 3 In+ ⇌ 2 In(s) + In3+                          K = ? given the following information: In3+ + 2e ⇌ In+                                      E° = –0.40 V In+ + e ⇌ In(s)                                       E° = –0.21 V

A reaction is reactant-favored at equilibrium. Will ratio of products to reactants in the cell be the same as equillibrium ?

7. Given the following information, find K, for nitrous acid, HNO2. NO3 + 3H+ + 2e HNO₂ + H₂O E° = 0.940 V E' = 0.433 V

Write the net ionic equations that occur in the following cells: Pb| Pb(NO3)2 ||AGNO3 | Ag Zn | ZnCl, || Pb(NO;)2 | Pb Pb| Pb(NO3)2 || NiCl, | Ni

The equilibrium constant K for the overall reaction that takes place in the cell Pt|Sn2+, Sn4+||Ag+|Ag at 298 K is?