Question 30 [2 marks] What is the equilibrium constant for the following reaction at 298 K which has E= +0.78 V? Fe...
A reaction has an equilibrium constant of 6.1×103 at 298 K. At 727 K , the equilibrium constant is 0.78. a.) Find ΔHorxn for the reaction. (in kJ)
What is the equilibrium constant for the following reaction at 298 K? 2 Ag+(aq) + 2 I-(aq) → I2(s) + 2 Ag(s) Eº = +0.265 V Group of answer choices 2.99 x 104 1.60 x 107 9.04 x 108 87.9 7.73 x 103 Using data from the reduction potential table below and the reaction 2 Ag(s) + Pt2+(aq) → Pt(s) + 2 Ag+(aq) Eº = 0.38 V calculate the standard reduction potential of the half-reaction Pt2+(aq) + 2 e- →...
cell = 0.74 V. Calculate the equilibrium constant, K. For the following redox reaction at 25 °C, E° Cd(s) + Cu 2+ (aq) → Cd 2+ (aq) + Cu(s)
B3438 QUESTION 24 What is the equilibrium constant (K) at 350 K for the following reaction? (R= 8.314 J/K.mol, F = 96,500 C-moll) Sn2+ (aq) + Fe(s) Sn(s) + Fe2+(aq) E cell = 0.35 V O 7.1 x 10-11 1.2 x 1010 1.2 x 105 8.6 x 10- 2.3 1023 QUESTION 30 A chemist adds substance A and B to a reaction flask and allows equilibrium to establish A+B=CKc= 1.5 x 10-25 Which of the following describe the contents of...
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.
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
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.
6. At 298 K, the equilibrium constant for the below reaction is 4.17 x 103. What is the concentration of Clat equilibrium? Pb2+ (aq) + 2 C1" (aq) = PbCl2 (5) (a) 20.2 M (b) 0.078 M (c) 10.1 M (d) 0.039 M
A reaction has an equilibrium constant of 7.1×103 at 298 K. At 711 K , the equilibrium constant is 0.72. Find ΔHorxn for the reaction.
A reaction has an equilibrium constant of 8.3×103 at 298 K. At 707 K , the equilibrium constant is 0.48. Find ΔHorxn for the reaction.