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5. The first step in the commercial production of titanium metal is the reaction of TiO2...
5. The first step in the commercial production of titanium metal is the reaction of TiO2 with chlorine and graphite: TiO2 (s) + 2 Cl2 (g) + 2 C(s) TiCl4 (1) + 2 CO (g) Calculate AGº for the reaction. Substance AG? (kJ/mol) Substance AG (kJ/mol) C(s) 0 TiCl4 (1) -804.2 CO (g) -110.5 TiO2 (s) -944.0 Cl2 (8) 121.3
The first step in the commercial production of titanium metal is the reaction of rutile (TiO2) with chlorine and graphite: TiO2(s) + 2Cl2(g) + 2C (s) TiCl4(l) + 2CO (g) Use the following data to calculate Keq for this reaction at 25° C. Formula ?H°f (KJ/mol) S° (J/K mol) TiO2(s) -944.0 50.6 Cl2(g) 0 223.0 C (s) 0 5.7 TiCl4(l) -804.2 252.3 CO (g) -110.5 197.6
AH-116.4 kJ/mol 4. Consider the following reaction: NH.NO, (s) N20 (8) + 2 H20 (g) Calculate AGⓇ for the reaction. Substance S” (J/mol K) NH.NO, (3) 151 N:0 (8) 220 H:0 (9) 183 5. The first step in the commercial production of titanium metal is the reaction of Tio: with chlorine an graphite: TiO2 (s) + 2 Cl: (g) + 2C (5) Tici: (1) + 2 CO(g) Calculate AGº for the reaction. Substance AG? (kJ/mol Substance AG® (kJ/mol) C(s) TiCl...
Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. Calculate ΔrG° and K at 891°C. Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. TiO2 (s) + 3 C(s) + 2 CO(g) + TiC(s) Compound AfGº (kJ/mol) TiO2 (s) -728.24 TiC(s) -159.09 CO(g) -214.92 a Calculate A,Gº and K at 891 °C. AG = kJ K=
step by step please Cis. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) AHºf AG°f S (J/K- Substance KkJ/mol KkJ/mol mol) C(s. 1.88 2.84 2.43 diamond) lo 6 5.69 graphite) C2H2(8) 226.7 209.2 200.8 C2H4 (8) 52.30 68.11 219.4 C2H6 (g) -84.68 -32.89 229.5 CO(g) - 110.5 -137.2 197.9 CO2(g) -393.5 394.4 213.6 H2(g) 130.58 O2 (g) 0 205.0 H20 (1) 285.83 -237.13 69.91 0 The combustion of acetylene in the presence of excess oxygen yields carbon dioxide and...
3 attempts left Check my work Enter your answer in the provided box. Calculate AG for the reaction at 25°C. 2C6H61) + 1502(8) 12C028) + 6H20(1) agº = kJ AH° (kJ/mol Agº (kJ/mol) sº (J/K mol) 5.69 2.4 Substance C(graphite) C(diamond) CO(g) CO2(g) CO2(aq) C0,- (aq) O(g) O2(8) O3(aq) O3(8) H20(1) CH 1.90 -110.5 -393.5 -412.9 -676.3 249.4 2.87 --137.3 -394.4 -386.2 --528.1 230.1 0 16.3 163.4 -237.2 124.5 197.9 213.6 121.3 -53.1 160.95 205.0 110.88 237.6 -12.09 142.2 -285.8...
Purification of Ni metal can be facilitated by its ability to react with carbon monoxide. Ni(s) + 4CO(g) --> Ni(CO)4(g) Substance: Ni(s) CO(g) Ni(CO)4(g) S°(J/K•mol): 30.1 197.9 410.6 DH° (kJ/mol): 0 -110.5 -602.9 What is DG° for this reaction? A) –437.9 kJ/K•mol B) +437.9 kJ/K•mol C) +38.4 kJ/K•mol D) –38.4 kJ/K•mol E) –438.2 kJ/K•mol
step by step please 1/1 pts Question 12 Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) Substance ΔΗ°F (kJ/mol) AGOF (kJ/mol S (J/K- mol) 1.88 2.84 2.43 5.69 C (s, diamond) C(s. graphite) C2H2(g) C2H4 (8) C2H6 (g) CO(g) CO2 (g) H2(g) O2(g) H2O(0) 226.7 52.30 -84.68 -110.5 -393.5 0 0 -285.83 209.2 200.8 68.11 219.4 -32.89 229.5 -137.2 197.9 -394.4 213.6 0 130.58 0 205.0 -237.13 69.91 The value of AH°for the catalytic hydrogenation of acetylene to ethane,...
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. AG® (kJ/mol) M,0,0) = 3M(s) +20,(g) -8.30 Substance M304(5) M(S) O2(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? AGix= kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? KE What is the equilibrium constant of this reaction, as written, in the forward direction at 298...
A metal object at 54.0 oC is heated by gaining 30.2 kJ of heat from the environment. The heat capacity, C, of the metal object is 6.30 kJ/ oC When 11.53 g C2H6O (g) is reacted according to the following equation, 368 kJ of heat is released. What is the ΔH of the reaction? C2H6O (g) + 3O2(g) --> 2CO2(g) + 3H2O (l) When 2.45 g of CH3OCH3 is burned at constant Pressure, 77.42 kJ of heat is given off. What is...