Calculate AS°sys for the below chemical reaction using the provided AS° values. CacO3 (s, calcite) + 2 HCI (g) → CaCl2 (s) + CO2 (g) + H2O (1) Substance AS° (J/(mol•K)) HCI (g) 186.69 CaCl2 (s) 104.6 CaCO3 (s, calcite) 92.88 CO2 (g) 213.6 H20 (1) 69.91 H2O (g) 188.83 O 227.5 J/(mol•K) O -78.15 J/(mol•K) -101.6 J/(mol•K) O 40.77 J/(mol•K) O 108.5 J/(mol•K)

Calculate AS°sys for the below chemical reaction using the provided AS° values. CacO3 (s, calcite) + 2 HCI (g) → CaCl2 (s) + CO2 (g) + H2O (1) Substance AS° (J/(mol•K)) HCI (g) 186.69 CaCl2 (s) 104.6 CaCO3 (s, calcite) 92.88 CO2 (g) 213.6 H20 (1) 69.91 H2O (g) 188.83 O 227.5 J/(mol•K) O -78.15 J/(mol•K) -101.6 J/(mol•K) O 40.77 J/(mol•K) O 108.5 J/(mol•K)

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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Please answer Question #17.
8. Nitric oxide reacts with chlorine to form NOCI. The data refer to 298 K. 2NO(g) + Cl₂(g) → 2NOCI(g) Substance: NOCI(g) 51.71 AH° (kJ/mol): 66.07 AG°f(kJ/mol): S°(J/K-mol): 223.0 261.6 What is the value of AG for this reaction at 550 K? Is the reaction spontaneous or not? NO(g) 90.29 86.60 210.65 A) -143.76 kJ, nonspontaneous B) -78.78 kJ, spontaneous C) -22.24 kJ, nonspontaneous D) -10.56 kJ, spontaneous E) 66600 kJ, no idea Cl2₂(g) 0 0
Determine AS° for 2 03(g) → 3 O₂(g). Substance S° (J/mol.K) 03 (9) 239 O2 (g) 205 - J/mol · K
8
Calculate AS° for the reaction SiClĄ(g) + 2Mg(s) → 2MgCl2(s) + Si(s) Substance SICI,(8) Mg(s) MgCl2(s) Si(s) S° / (J/K'mol) 330.73 32.68 89.62 18.83 471 J/K -198 J/K 255 J/K -255 J/K O 198 J/K
2) a)Determine AGX"° values for the following Combustion reactions at 25°C b) Decide whether this reaction is spontanious at 25°C or not CH:(g) + 02(g) CO:(g) + H;0 (1) AH (kJ/mol) s° (kJ/mol) CH4 -74.87 0.186 0.205 CO2 H,O -393.51 0.214 -285.83 0.070
Given the reaction: 4 Fes) + 3 02(g) - 2 Fe2031s) Delta H = -822.16 kJ --> What is Delta H for the reaction below? ----> 2 Fes) + 3/2 O2(2) + 822.16 kJ + 411.08 kJ 411.08 kJ O + 1644 kJ
Calculate AS°, in J/K for the following reaction at 373K. (rxn) CO(g) + H2O(g) → CO2(g) + H2(g) ΔΗ ο (rxn) = -4.1 x 104 J AS univ = 56 J/K
Consider the following reactions and predict the AS°: I. C6H6(s) – C6H6(1) 2 SO2(g) + O2(g) –→ 2 SO3(g) II. AS should be negative for I and positive for II. AS® should be positive for I and positive for II. AS should be negative for I and negative for II. AS should be positive for I and negative for II.
3.
For the reaction: CuS (s) + H₂(g) → H₂S (g) + Cu (s) Given: ΔS ⁰ (CuS) = 66.5 J/mole-K ΔHf ⁰ (CuS) = -53.1 kJ/mol ΔS ⁰ (H₂S) = 205 J/ mole-K ΔHf ⁰ (H₂S) = -20.6 kJ/mol ΔS ⁰ (Cu) = 33.3 J/ mole-K ΔH f ⁰ (Cu) = 0.0 kJ/mol ΔS ⁰ (H₂) = 131 J/ mole-K ΔH f ⁰(H₂) = 0.0 kJ/mol The standard free energy of the reaction ΔG ⁰ rxn is A) -37.9 kJ/mole B) 44.6 kJ/mole C) -20.3 kJ/mole D) +20.3kJ/mole and spontaneous E) +37.9 kJ/mole
One of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3(g) ⇒ NO2 (g) + O2(g) Substance and State AGf (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate ΔG° (at 298 K) for this reaction. AG = -198 kJ b Calculate K (at 298 K) for this reaction. K =