Consider the reaction:
FeO (s) + Fe (s) + O2(g) → Fe2O3
(s)
Given the following table of thermodynamic data at 298 K:
Substance | ΔHf° (kJ/mol) | S° (J/K⋅mol) |
FeO (s) | -271.9 | 60.75 |
Fe (s) | 0 | 27.15 |
O2 (g) | 0 | 205.0 |
Fe2O3 (s) | -822.16 | 89.96 |
The value K for the reaction at 25 °C is ________.
A.370
B.7.1 x 1085
C.3.8 x 10-14
D.5.9 x 104
E.8.1 x 1019
Consider the reaction: FeO (s) + Fe (s) + O2(g) → Fe2O3 (s) Given the following...
Given the following chemical reaction and standard thermodynamic quantities in the table, FeO(s) + Fe(s) + O2(g) → Fe2O3(s) FeO(s) Fe(s) O2(g) Fe2O3(s) ∆H°f (kJ/mol) −271.9 0 0 −822.16 ∆S° (J/mol∙K) 60.75 27.15 205.0 89.96 at 298 K, ∆G° for this reaction is [ Select ] ["‒490 kJ", "‒611 kJ", "59.9 kJ", "59926 kJ"] , and the reaction is ...
Consider the reaction: FeO (s) + Fe (s) + O_2 (g) rightarrow Fe_2O_3 (s) Given the following table of thermodynamic data, Substance Delta H_f degree S degree FeO (S) -271.9 kJ/mol 60.75 J/mol - K Fe (s) 0 27.15 O_2 (g) 0 205.0 Fe_2O_3 (S) -822.16 89.96 determine the temperature (in degree C) above which the reaction is nonspontaneous.
can someone please help me step by step? i get confused when trying to input values into the delta g equation and don't get the right answer Question 10 FeO ()Fe (s)O2 (8)Fe203 (s) Given the following table of thermodynamic data at 298 K: Substance | △Hf (kj/mol) | So (J/K-mol) FeO (s) Fe (s) O2 (8) Fe203 (-822.16 -271.9 60.75 27.15 205.0 89.96 The value K for the reaction at 25 °C is Selected Answer7.1x 1085 7.1x 1085
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)> Fe20,(s) ДН/ (kJ/mol) So (J/K-mol) FeO(s) -271.9 60.75 Fe(s) Fe203 (a) 618.1°C 27.15 205.0 89.96 0 -822.16 (b) 756.3°C (c) 1235°O (d) 2439°C (e) spontaneous at all temperatures Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)>...
You are given the following thermodynamic data. 2 Fe(s) + 3/2 O2(g) → Fe2O3(s) ΔH° = -823 kJ 3 Fe(s) + 2 O2(g) → Fe3O4(s) ΔH° = -1120. kJ Calculate the ΔH° for the following reaction. 3 Fe2O3(s) → 2 Fe3O4(s) + ½ O2(g)
Using standard heats of formation calculate AH for 4 FeO (s) + O2 (g) 2 Fe Os (s) AHr of FeO (s) - -272.0 kJ/mol 5 AH'T of Fe2O3 (s) = -825.5 kJ/mol
Calculate H for this reaction: FeO(s) + CO(g) Fe(s) + CO2(g) Given: Fe2O3(S) + CO(g) 2FeO(s) + CO2(g) H= +38 kJ Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) H= -28 kJ
3) Answer all parts of the following question. a. The reaction: Al(s) + Fe2O3(s) → Fe(s) + Al2O3(s) has ΔH = -847.6 kJ and ΔS = -41.3 J/K at 25°C. Calculate ΔG and determine if it is spontaneous. 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 c. Find ΔSsurr and predict whether or not this reaction will be spontaneous at 398 K. NH3(g)...
5. Using standard heats of formation, calculate AH for 4 FeO (s) + O2(g) → 2 Fe2O3 (s) AH1 of FeO (s) = -272.0 kJ/mol AHºf of Fe2O3 (s) = -825.5 kJ/mol 3. Given 3 C (s) + 4 H2(g) → C3H8 (9) AH = -103.85 kJ/mol C(s) + O2(g) + CO2(g) AH = -393.5 kJ/mol H2 (g) + 12 O2(g) → H2O (1) AH = -285.8 kJ/mol find AH for C3H8 (g) + 5 O2(g) → 3 CO2 (g)...
Consider the four reactions listed below for the next question. 1. FeO(s)+CO(g)<->Fe(s)+Co2(g) K=0.403 2. 2C(s)+O2(g)<->2CO(g) K=1x10at16 power 3. 2Cl2(g)+2H2O(l)<->4HCl(aq)+O2(g) K=1.9x10 at-15 power 4. C(s)+2H2(g)<->CH4(g) K=27.5 a.Which reaction has the smallest tendency to occur? 1. Reaction a 2. Reaction b 3. Reaction c 4. Reaction d