5. (18 pts: 6 pts each) For a reaction:N2O4 (g) 2 NO2 (g), the thermodynamicconstants at 25°C are listed in the table below:CompoundNO2 (g)AH (kJ/mol)AG+ (kJ/mol)So (J/mol·K)33.2051.30240N2O4 (g)9.1697.82304.2(a) What is the equilibrium constant K of this reaction at 25°C?(b) In a closed container, the partial pressures of N2O4 (g) and NO2 (g) initially are 0.10 atmand 0.10 atm, respectively. Is this reaction spontaneous (i.e. moving forward) at 25°C?(c) Continued from (b), what will be the partial pressures of N2O4 and NO2 when the systemreaches equilibrium? (Help: Root of a quadratic equation is in Supporting Table-1.)

Given: T=298.15KΔHf°,kJ/molS°,J/molKN2O4(g)9.16304.2⇌2NO2(g)33.20240 A. Equilibrium…

Answered: 5. (18 pts: 6 pts each) For a reaction:…

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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3.) Consider the reaction below. Reaction: AH°r (kJ/mole) 2 ICI (£) 17.78 L. (g) 247.551 l16.135 223.066 (/mole K) Which explains the outcome when 0.45 mol ½, 0.45 mol Cl2, and 2.42 mol ICl are added to a 2.0L flask at 25°C? A. [ICI] decreases B. [ICI] increases C. both [b] and [CL] increase D. at equilibrium Keywords: reaction quotient (Q), initial concentration(s), equilibrium concentration(s), equilibrium constant, forward reaction, reverse reaction, Q K. Q= K Concepts: Reaction Quotient, Chemical equilibrium
Calculate AH for the reaction 4 NH3 (g) + 5 02 (g) à 4 NO (g) + 6 H2O (g), from the following data N2 (g) + 02 (g) -> 2 NO (g) Ne (g) + 3 H2 (9) -> 2 NH3 (g) 2 H2 (9) ?H = -120.0 kJ ?H = -90.0 kJ + O2 (g) -> 2 H20 (g) ?H = -400.0 kJ Select one: O a. -1620 kJ/mol O b. -1260 kJ/mol O c. -430 kJ/mol O d. -860 kJ/mol
Calculate the Gibbs free energy change (∆GRXN) in kJ that occurs when one mole of solid iron (III) oxide is produced from solid iron and water. (One decimal place) The unbalanced chemical equation for the process is: Fe (s) + H2O (g) --> Fe2O3 (s) + H2 (g)
Compound SO; (g) SO₂ (g) NH3 (g) NO (g) H₂O (9) Consider the following reaction at 25 °C: 5 SO3(g) + 2 NH³(g) → 2 NO(g) + 5 SO₂(g) + 3 H₂O(g) Given the information in the table, calculate AH° for the reaction. AHf (kJ/mol) -396 -297 -46 90.4 -241.8 Sf (J/mol-K) 256 248 192.5 210.6 188.7
The following questions refer to the reaction below. N2(g) + O2(g) 2 NO(g) AH° = 181.8 kJ 1. This reaction is Oexothermic Oendothermic 2. Heat is Oreleased Oabsorbed by the chemicals in this reaction. 3. Calculate AH° for the reaction YouTube 4 NO(g) 2 N2(g) + 2 O2(g) AH° = kJ 4. Calculate the standard heat of formation of NO. AH°t kJ %3D 5. Calculate the amount of heat transferred when 3.000 g of N2 are reacted with excess O2 gas.
7. Calculate the standard enthalpy change at 25°C for the reaction CH, (g) + 2 H₂S (g) →→ CS₂ (1) + 4H₂(g) The values of AH'at 298 K for reactants and products are: Adf 298/kJ mol¹: CH4(g) = -74.8; H₂S (g)=-20.6; CS₂ (1)=+89.7; H₂(g) - 0.
Methane-producing bacteria convert liquid acetic acid (CH3CO₂H) into CO₂(g) and CH₂(g). AS° ΔΗ, Ο (kJ/mol) (J/mol.K) CH3CO₂H (1) -484.5 159.8 CO₂(g) -393.5 213.8 CH₂(g) -74.8 186.2 Calculate AHOrxn = kJ Calculate AG rxp = (round to 3 sig figs) Is this process endothermic or exothermic under standard conditions? Is the reaction spontaneous under standard conditions? kJ (round to 3 sig figs)
please answer all the questions given in the picture.
Use the molar DHf° under the formulas to calculate DH°rxn for the equations as balanced: 1. 2B2H6(g) + 3CO2(g) --> 2B2O3(s) + 3CH4(g) ΔH°rxn = _______ kJ ΔH°f = +36 –394 –1274 –75 kJ/mol exo ? endo_thermic 2. 2P2O5 + 2CaC2 -->P4 + 2CaCO3 + 2CO2 ΔH°rxn = _______ kJ ΔH°f = –1505 –59 ___ –1207 –394 kJ/mol exo ? endo_thermic 3. 2Na2CrO4(s) + 10HCl(g) --> 4NaCl(s) + 3Cl2(g) + Cr2O3(s) + 5H2O(l) ΔH°f = –1342 –92 –411 ___ –1140 –286 kJ/mol ΔH°rxn = _______ kJ exo ? endo_thermic
Calculate the Gibbs free energy change (∆GRXN) in kJ that occurs when one mole of solid iron (III) oxide is produced from solid iron and water. (One decimal place) The unbalanced chemical equation for the process is: Fe (s) + H2O (g) --> Fe2O3 (s) + H2 (g)
Methane-producing bacteria convert liquid acetic acid (CH³CO₂H) into CO₂(g) and CH₂(g). AS° ΔΗ, Ο (kJ/mol) (J/mol.K) CH3CO₂H (1) -484.5 159.8 CO₂(g) -393.5 213.8 CH₂(g) -74.8 186.2 Calculate AHºrxn = kJ Calculate AG, = rxn (round to 3 sig figs) Is this process endothermic or exothermic under standard conditions? Is the reaction spontaneous under standard conditions? kJ (round to 3 sig figs)
Enter your answer in the provided box. 0 Calculate AG for the reaction at 25°. You will have to look up the thermodynamic data. 2C₂H6(g) + 70₂(g) → 4CO₂(g) + 6H₂O(1) kJ/mol

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