The reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking,2 FeO3(s)4Fe(s) + 302(g)is driven by the high-temperature combustion of coke, a purified form of coal:C(s) + O2(g) → CO₂ (g)->11✓12Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are -447. kJ/mol and -818. kJ/mol, respectively.Calculate the minimum mass of coke needed to produce 7800. kg of pure iron.Round your answer to 2 significant digits.kg5

Step 1:Answer Minimum mass of coke 1.26×10^4 kg Step 2 Mole = mass / molar mass Molar mass of C =…

Answered: The reduction of iron(III) oxide…

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...

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The equilibrium constant of a system, K, can be related to the standard free energy change, AGO, using the following equation: AG-RT In K where I is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K.mol). Under conditions other than standard state, the following equation applies: AG = AG° + ᎡᏆ ln Q In this equation, Qis the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene, C₂ H2, can be converted to ethane, C₂H6, by a process known as hydrogenation. The reaction is C₂H₂(g) + 2H₂(g) = C₂H6(g) Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction? 9A V—| ΑΣΦ Substance Express your answer using two significant figures. ►View Available Hint(s) t C₂ H₂(g) H₂(g) C₂H6(g) P ? Review | Constants | Periodic Table AG (kJ/mol) 209.2 0 -32.89
Calculate the change in internal energy (in kcal) for the reaction Cl2(g) + 7/2 O2(g) = Cl₂O7(g) at 25 °C, given that the gases are ideal. The enthalpy, AH, for the formation of Cl₂O7(g) is 63.4 kcal mol- ¹ at 25 °C.
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. AG°r(kJ/mol) Substance M20(s) -6.00 M,0(s) = 2 M(s) + 0,(g) M(s) O2(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? kJ/mol AG:xn What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? K = What is the equilibrium pressure of O2(g) over M(s) at 298 K? atm Po,
At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4B(g) 2 C(g) + 3D(g) were found to be PA = 4.71 atm, PB = 4.26 atm, Pc = 5.75 atm, and P = 4.58 atm. What is the standard change in Gibbs free energy of this reaction at 25 °C? AGrxn = kJ mol
a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq. A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species. You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?
A 65.0 g piece of gold at 650 K is dropped into 162 g of H2O(l) at 298 K in an insulated container at 1 bar pressure. CP,m for Au and H2O at 298 K are 25.4 and 75.3 J⋅K−1⋅mol−1, respectively. Calculate the temperature of the system once equilibrium has been reached. Assume that CP,m for Au and H2O are constant at their values for 298 K throughout the temperature range of interest.
G.59.
Make a non-spontaneous process spontaneous A process that is nonspontaneous can be made spontaneous by coupling it with another process tha is highly spontaneous. The coupling of nonspontaneous reactions with highly spontaneous ones is important in biological system. The oxidization of glucose, for example, is highly spontaneous: C6H12O6(s) + 60₂(g) → 6 CO₂(g) + 6 H₂O(1) Spontaneous reactions such as this ultimately drive the nonspontaneous reactions necessary to sustain life. Can you use Gibbs free energy, enthalpy, and entropy to argue this reaction is highly spontaneous?
A chemist fills a reaction vessel with 0.137 g calcium phosphate (Ca, (PO,) solid, 0.349 M calcium (Ca ) aqueous solution, and 0.240 M phosphate (Po,") 3- POA aqueous solution at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: Ca3 (PO4),(s) → 3Ca (aq) + 2PO, (aq) 4. Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ
Calculate the standard Gibbs reaction energy for the reaction at 298 K, 2CH3CHO(g) + O2(g) - > 2CH3 COOH(I) Given the following data, Sm\deg (CH3CHO(g )) = 250.30 J K-1 mol-1 Sm\deg (O2(g)) = 205.10 JK -1 mol-1 Sm\deg (CH3COOH(l))=159.80~K-1~mol-1\backslash Delta fHm\deg (CH3CHO(g))=-166.20~kJ~mol-1\backslash Delta fHm\deg (O2(g)) = 0.00 kJ mol-1 \Delta fHm\ deg (CH3COOH(I)) = 484.50 kJ mol-1

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