ΔGr for the reaction Fe2O3(s) + 3 H2(g) ⇌ 2 Fe(s) + 3 H2O(g) is 45.0 kJ/mol when there is 1.5 mols Fe2O3, 0.75 mols H2, and 0.15 mols Fe in a 1.0 L flask at 25.0 oC. What is the concentration of H2O in the flask? (Hint: ΔfGo values are available below the periodic table at the end of the exam.)
a. 0.15 M
b. 0.67 M
c. 0.26 M
d. 0.75 M
e. 0.030M
ΔGr for the reaction Fe2O3(s) + 3 H2(g) ⇌ 2 Fe(s) + 3 H2O(g) is 45.0...
Determine the value of AG for the following reaction: Fe2O3 (s) + 3 H2(g) → 2 Fe(s) + 3 H2O(g) Fe2O3(s) H2(g) Fe(s) H2O(g) AHf (kJ/mol) -824.2 0 0 -241.8 Sº (J/K mol) 87.4 130.6 27.3 188.8
15. Determine the standard enthalpy of formation of Fe2O3(s), 2Fe(s) + 1.5 02 (g) → Fe2O3(s) given the thermochemical equations below. (4 points) AFH° = +160.9 kJ/mol-rxn Fe(s) + 3 H20(8) - Fe(OH)3(s) + 3/2 H (9) H2(g) + 1/2 O2(g) → H2O(6) Fe2O3(s) + 3 H2O(0) - 2 Fe(OH)3(8) A-H° = -285.8 kJ/mol-rxn A,Hº = +288.6 kJ/mol-rxn
5 Determine the standard enthalpy of formation of Fe2O3(s) given the thermochemical equations below. 2Fe(s) + 3/2 O2(g) → Fe2O3(s) AH(Fe2O3) = ? Fe(s) + 3 H2O() Fe(OH)3(s) + 3/2 H2(g) AH° = +160.9 kJ/mol-rxn H2(g) + 1/2O2(g) → H2O(1) A.H° = -285.8 kJ/mol-rxn Fe2O3(s) + 3 H2O(1) ► Fe(OH),(s) A,Hº +288.6 kJ/mol-rxn
The following reaction is at equilibrium: 2 Fe(OH)3(s) ↔ Fe2O3(s) + 3 H2O(g); Ho > 0. Which of the following changes will result in a decrease in the concentration of water (gas)? 1. Increasing the temperature. 2. Decreasing pressure. 3. Adding a catalyst. 4. Adding some Fe(OH)3. 5. Decreasing the volume. 6. Removing some Fe2O3.
For the reaction. Fe2O3 (s) + 3 H2(g) <=> 2 Fe(s) + 3 H20(8), AGⓇ - 43 kat 25 °C and AH - 100k. Which of the following is completely true about the relationship between AG and T for this reaction? A. AGO when T> 525 K B.AG > when T> 525 K C. AGO when T> 0.5K DAGO when T < 520 K E. AG < when T <0.5 K
37. Balance the following equations: a. PbO2(s) —>PbO(s) + O2(g) b. Fe(OH)3(s) —>Fe2O3(s) +H2O(s) C. (NH4)2CO3(s) —>NH3(g)+H20(g) + CO2(g) d. CaCl2(aq) + H2SO4(aq) — CaSO4(s) + HCl(aq) 761
2.Calculate the enthalpy of reaction for the following reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5 kJ/mol
b Using the equation: Fe2O3(s) + 3 CO(g) + 2 Fe(s) + 3 CO2(g) How many moles of Fe2O3 are required to produce 45.9 mol of Fe? How many grams of CO are required to produce 45.9 mol of Fe? 1 pt nFe2O3) - mol 1 pt m(CO) -
2. Determine: 2 Fe2O3 (s) + 3 C(s) + 3 CO2 (g) + 4 Fe (s) Given: 2 Fe (s) + 3/2 O2 (g) → Fe2O3 (s) C(s) + 1/2 O2 (g) → CO (g) CO (g) + 1/2 O2 (g) → CO2 (g) AH = -822.2 kJ AH = -110.5 kJ AH = -283.0 kJ
1.00 mol Fe(s) and 3.00 mol H2 (g) were placed into a 5.00 L reaction vessel where the Kc for the reaction below is 0.825 at 400K. What is the concentration of hydrogen gas at equilibrium? Fe2O3 (s) + 3H2 (g) <----> 2Fe (s) + 3H2O (g)