4. Thermodynamic data for C(graphite) and C(diamond) at 298 K is given in the table below. 6) Will produc ΔΗ (KJ/mol) S° (J/mol K) C(graphite) 0.0 5.740 C(diamond) 1.895 2.377 a) Calculate AH° and AS° and AG° for the transformation of one mole of graphite to diamond at 298 K. AH'rxn={[he products] - WF Reactants +298 K.

4. Thermodynamic data for C(graphite) and C(diamond) at 298 K is given in the table below. 6) Will produc ΔΗ (KJ/mol) S° (J/mol K) C(graphite) 0.0 5.740 C(diamond) 1.895 2.377 a) Calculate AH° and AS° and AG° for the transformation of one mole of graphite to diamond at 298 K. AH'rxn={[he products] - WF Reactants +298 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...

See similar textbooks

Similar questions

3:18 Question 9 of 16 Which of the following phase changes is not spontaneous at room temperature? Assume only the first phase is initially present. A) H₂O(g) → H₂O(1) B) H₂O(s) → H₂O(g) C) H₂O(s) → H₂O(l) D) H₂O(g) → H₂O(s) E) They are all spontaneous. Submit Tap here or pull up for additional resources
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)
Calculate the AS° for the given reaction. + Cazs(PO4)2(0) 2+ Ca (ag) + PO43 (ag) molar ratio of the balanced chemical equation: Caz(PO4)2(0) 2+ Ca (ag) PO,3- Substance (at -53.1 -222.0 S° ( J/mol · K) 241.0 ES" (product) %3D ES (reac tan t) AS°, rxn
One of the reactions that destroys ozone in the upper atmosphere is NO(g) + 03 (g) ⇒ NO2 (g) + O₂(g) Substance and State ▲Gƒ° (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate AG (at 298 K) for this reaction. l\G° = Submit KJ
QUESTION 1 The heating curve below was generated by measuring the temperature of a compound which is a solid at point A as heat was added at a constant rate. The line segment_(1)_ is related to the heat of fusion of the solid and the line segment_(2)_ is related to the heat capacity of the compound in the liquid state. temperature (K) OA. (1): AB (2) : BC OB. (1): BC (2): CD B A C D heat added (J) E F
When nitric acid reacts with hydrazine (i.e. dinitrogen tetrahydride), nitrogen gas and water are formed. The temperature is constant at 25°C.4 HNO3(aq) + 5 N2H4(l) " 7 N2(g) + 12 H2O(l)Substance ΔHf° (kJ/mol) S° (kJ/mol K)HNO3 (aq) –133.9 0.2669H2O (l) –285.8 0.0700N2 (g) 0 0.1916N2H4 (l) +50.6 0.1212a. Calculate ΔH° (in kJ/mol) and ΔS° (in kJ/mol K).b. Calculate ΔG° (in kJ/mol).c. Determine K for this reaction.
b How does A,G° vary with temperature? 2 N2 (g) + O2 (g) → 2 N20(g) Compound A,H° (kJ/mol) S° (J/mol · K) A,G' (kJ/mol) N2 (g) 191.56 02 (g) 205.07 N20(g) 82.05 219.85 104.20 O A,G° increases when the temperature increases. O 4,G° decreases when the temperature increases.
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)
Calculate AG° and AS°at 25 °C for the following fermentation reaction: 2. C,H1206(aq) → 2C2H;OH(aq) + 2C02(9) AG° (C,H1206, aq) = -910.4 kJ/mol AH°; (C,H1206,aq) = -1273.3 kJ/mol AG°; (C,H5OH,aq) = -181.64 kJ/mol AH°;(C2H50H,aq) = -288.3 kJ/mol AG°; (CO2,g) = -394.36 kJ/mol AH° (CO2,g) = -393.51 kJ/mol Note: Be mindful that we read all of your submissions individually. Corresponding deductions will be applied to students with the same output if plagiarism is detected.
1. Using Hess's Law, calculate AH for this reaction: (T: 5) CIF(g) + F₂(g) ---> CIF3(g) given: 2CIF(g) + O₂(g) ---> Cl₂O(g) + F₂O(g) ΔΗ = 167.4 kJ 2CIF3(g) + 202(g) ---> Cl₂O(g) + 3F₂O(g) AH = 341.4 kJ 2F2(g) + O₂(g) ----> 2F₂O(g) ΔΗ = -43.4 kJ
Consider the reaction 2502(g) + O2(g)- -2S03(g) Using the standard thermodynamic data in the tables linked above, calculate AGn for this reaction at 298.15K if the pressure of each gas is 25.91 mm Hg. ANSWER: kJ/mol
Is the following chemical reaction exothermic or endothermic? 31 (aq) + H3AS04(aq) + 2H* (aq) 13 (aq) + H3ASO3(aq) + H2O() AH°F(kJ/mole) S° (J/mole*K) Substance or ion -55.19 180.7 I (aq) -345.69 212.34 H3ASO4(aq) -11.23 11.09 H* (aq) 69.77 -89.6 13 (aq) H3ASO3(aq) -301.27 199.78 -285.8 69.95 H20 (1) endothermic then exothermic All I know is the reaction is cold to the touch