Determine the equilibrium constant at 298 K for the reaction: Zn (s) + Ni2+ (aq) Zn2+ (aq) + Ni (s) (Hint: Start with the E°)
A) (4.1 ± 0.1) x 10 3
B) (1.7 ± 0.1) x 10 17
C) (9.3 ± 0.1) x 10 8
D) (6.4 ± 0.1) x 10 -6
---------------------------------------------------------------------------------------------------------------
Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g). Assume ΔH°rxn = 41.0 kJ/mol for all temperatures in this problem. If Kp = 5.10 at 700K, at what temperature will Kp = 2.5?
A) (692 ± 2) K
B) (685 ± 2) K
C) (779 ± 2) K
D) (636 ± 2) K
--------------------------------------------------------------------------------
For the process involving compound A: A(s) → A(l), ΔH° = 8.8 kJ/mol, and ΔS° = 36.4 J/mol•K. What is the melting point of compound A?
A) (31 ± 1) ℃
B) (-242 ± 1) ℃
C) (-31 ± 1) ℃
D) (242 ± 1) ℃
----------------------------------------------------------------------
Calculate ΔS° for the reaction of
N2O5(g) (S° = 355.3
JK-1mol-1) to make NO2(g)
(S° = 239.9 JK-1mol-1) and
O2(g) (S° = 204.8
JK-1mol-1) at 25°C.
A) (453.8 ± 0.5) J/K
B) (-249.2 ± 0.5) J/K
C) (-115.6 ± 1) J/K
D) (89.5 ± 0.5) J/K
(89.5 ± 0.5) J/K
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Determine the equilibrium constant at 298 K for the reaction: Zn (s) + Ni2+ (aq) Zn2+...
A reaction has an equilibrium constant of Kp=0.061 at 27 ∘C. Part A Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 6.98 kJ 0.839 kJ -6.98 kJ 0.628 kJ Part B Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K 298 K 158.7 K 6.762 × 103 K This reaction is nonspontaneous at all...
A) A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C. Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ B) Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) = -11.0 kJ; = -17.4...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) <----> (arrows both ways) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 391 K? Kp =_______
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 212 K? Kp =
Cell: Fe(s)| Fe2+(aq, 1M) | Cu2+(aq, 1M) | Cu(S) Calculated Values ΔG° = -nFE° = ΔH° - TΔS° ΔH° = -0.34905 J/C * 2 mols * 96485 C/mol = -67,356.18 J =67.36kJ ΔS° = 0.8597 x 10-3 J/C * 2 mols * 96485 C/mol = 165.89 J ΔG° =-67356.18 J – (298*165.9 J) = -116794.4 J = -116.79 kJ Theoretical Values ΔG⁰ = -(2 mols *96485 C/mol * 1.07 J/C) = -206.48 kJ ΔH⁰ = ΔS⁰ = Cell: Zn(s)| Zn2+(aq,...
Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH° = -304.2 kJ; ΔS° = -414.2 J/K
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -627 kJ and ΔS∘ = -153 J/K .
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -795 kJ and ΔS∘ = -349 J/K .
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -829 kJ and ΔS∘ = -367 J/K
20. Consider the reaction 2N2O5(g)4NO2(g) + O2(g) at 25 C for which the following data are relevant: Дн 13.30 kJ/mol 355.7 J/K mol N205 33.15 kJ/mol 239.9 J/K mol NO2 0 kJ/mol 204.8 J/K mol О2 Calculate AG° for the reaction at 25°C a. 1.35 x 105 kJ b. 94.7 kJ c. -29.0 kJ d. 135 kJ е. O kJ