The smelting of iron occurs in a blast furnace, as represented by the following overall equation. Step I 3Fe₂O3(s) + CO(g) → CO₂(g) + 2Fe3O4(s) A₁H° = -47.2 kJ Step II Fe3O4(s) + CO(g) → CO₂(g) + 3FeO(s) A,H° +19.4 kJ Step III FeO(s) + CO(g) - CO₂(g) + Fe(s) A,H° = -11.0 kJ The molar enthalpy of reaction for Fe₂O3(s) in the reaction represented by Step I is Record your 3-digit answer. Include sign; do not include units. Which steps in the above process can be represented by the following potential energy diagram? Potential Energy (kJ) Select one: O Step II only Reactants Steps I and III Steps I, II and III None of the above steps ◆ Products Reaction Pathway 15.7 kJ/mol Identify each of the following statements as true or false, as they pertain to the above 3 steps. In Step II, 6.47 kJ of energy are released when 1 mol of FeO(s) is produced. In Step III, 11.0 kJ of energy will be released when 1 mol of Fe(s) is produced. In Step III, 33.0 kJ of energy would be released if 3.00 mol of Fe(s) were produced.

The smelting of iron occurs in a blast furnace, as represented by the following overall equation. Step I 3Fe₂O3(s) + CO(g) → CO₂(g) + 2Fe3O4(s) A₁H° = -47.2 kJ Step II Fe3O4(s) + CO(g) → CO₂(g) + 3FeO(s) A,H° +19.4 kJ Step III FeO(s) + CO(g) - CO₂(g) + Fe(s) A,H° = -11.0 kJ The molar enthalpy of reaction for Fe₂O3(s) in the reaction represented by Step I is Record your 3-digit answer. Include sign; do not include units. Which steps in the above process can be represented by the following potential energy diagram? Potential Energy (kJ) Select one: O Step II only Reactants Steps I and III Steps I, II and III None of the above steps ◆ Products Reaction Pathway 15.7 kJ/mol Identify each of the following statements as true or false, as they pertain to the above 3 steps. In Step II, 6.47 kJ of energy are released when 1 mol of FeO(s) is produced. In Step III, 11.0 kJ of energy will be released when 1 mol of Fe(s) is produced. In Step III, 33.0 kJ of energy would be released if 3.00 mol of Fe(s) were produced.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given the following two measurements of the equilibrium constant for a reaction, calculate ΔH° for the reaction. (kJ/mol) T, °C K 30.0 5.2 x 103 50.0 15.4 x 104
What is ΔH for the following reaction?SiO2(s) + 2 Cl2(g) → SiCl4(l) + O2(g)
4. Consider the following: SiH 4(g) +2 O 2(g) <—> SiO 2(s) +2 H 2 O (l) Delta H^ 0 =-1516.86 kJ/mol a. Using the given information, calculate delta G^o for the reaction above at 25*C. b. Would you expect the reaction at 25*C to have an equilibrium constant greater than or less than 1 ? Explain.
Acetylene gas, C2H21g2, is used in welding. What is the maximum amount of useful work that can be accomplished under standard conditions by this reaction?
The thermite reaction, Fe2O3(s) + 2 Al(s) ---->2 Fe(s) +Al2O3(s), ΔH° = -851.5 kJ/mol, is one of the most exothermicreactions known. Because the heat released issufficient to melt the iron product, the reaction is used toweld metal under the ocean. How much heat is released permole of Al2O3 produced? How does this amount of thermalenergy compare with the energy released when 2 mol ofprotons and 2 mol of neutrons combine to form 1 mol ofalpha particles?
Example: At 25°C, calculate the AG° N₂+ 3H2 → 2NH3 • AG° N2(g) = 0 kJ/mol f • AG + H2(g) = 0 kJ/mol f • AG˚ NH 3(g) = -16.66 kJ/mol f a) 12.9 kJ b) -33.3 kJ c) -16.7 kJ d) -8.33 kJ e) Unsure sys for: AG sys =ΣnpG˚ products - Σn,G° reactants 60
Calculate ΔH° for the following reaction. CH4(g)+2O2(g)--> CO2(g)+2H2O(g) Use standard heats of formation from tables i provided below. not all are included.
The value of AH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na 20 2 with water is kJ. 2Na 20 2 (s) + 2H 20 (I) → 4NaOH (s) + O 2 (g) A 16.2 В 67.5 32.3 -126 E 8.08
Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction: 2Al(s) + Fe203(s) → Al203(s) + 2Fe(s) This reaction occurs when a mixture of powdered aluminum and iron(III) oxide is ignited with a magnesium fuse. The following enthalpies of formation are known: AH°; for Fe203(s) = -826 kJ AH°; for Al203(s) = -1676 kJ O 1251 kJ O 2502 kJ O-1251 kJ O 425 kJ 850 kJ O- 2502 kJ -850 kJ -425 kJ
Given the following equation, N20(g) + NO28) → 3 NO(g) AG°rxn = -23.0 kJ Calculate AG° rxn for the following reaction. 3N20(g) + 3NO2(g) 9 NO(g) -23.0 kJ 69.0 kJ -69.0 kJ -7.67 kJ 23.0 kJ
Balance the following equation and calculate its ΔSo in units of J mol-1 K-1. Fe(s) + H2O(l) → Fe3O4(s) + H2(g) Fe(s) - 27.3 J mol-1 K-1 H2O (l) - 70 J mol-1 K-1 Fe3O4 (s) - 146.4 J mol-1 K-1 H2 (g) - 130.7 J mol-1 K-1
Calculate the AG°rxn using the following information. AG°xn = ? 4 HNO3(g) + 5 N2H¾(1) → 7 N2(g) + 12 H20(1) AG°† (kJ/mol) -73.5 149.3 -237.1 -312.9 kJ -3.298 x 103 kJ +2.845 x 103 kJ +110.7 kJ -954.7 kJ