Using the data in the table calculate ΔGo (Delta Go) and equilibrium the constant Kp for the following reactions ( at 298.15K and 1bar).
a. 2NO(g) +O2 (g) <----> 2 NO2(g)
b. H2(g) + Cl2(g) <------> HCl(g)
Based on the equilibrium constant, does the equilibrium favo the reactants or the products?
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Using the data in the table calculate ΔGo (Delta
Go) and equilibrium the constant Kp for...
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,...
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A, G, for various hstances at 298.15 K and one har 1057 Substance Formula 4,6°/kJ-mol- acetylene ammonia C.H,() NH,(g) CHCI) Br(e) CH) C(s) C(s) CO (8) CO(g) 209.20 - 16.367 124.35 3.126 -17.15 2.900 benzene bromine butane carbon(diamond) carbon(graphite) carbon dioxide carbon monoxide ethane ethanol ethene glucose hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen peroxide iodine methane methanol CH(E) сHOH(1) CH (8) CH...
eNaICUrate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,G", for various substances at...
eNaICUrate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,G", for various substances at 298.15 K and one bar. 1057 Substance Formula 4,G"/kJ-mol acetylene сН.0 NH,(g) ammonia 209.20 benzene -16.367 с,н.Ф 124.35 bromine Br (g) 3.126 butane C,Hog) -17.15 carbon(diamond) C(s) 2.900 carbon(graphite) C(s) carbon dioxide cO(g) -394.389 carbon monoxide COg) -137.163 ethane СН, С Н, ОнФ сН. Ф C,H,0,(s) HBr(g) НСK -32.82 ethanol -174.78 ethene 68.421 glucose -910.52 hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide -53.513...
6-8 Using the table below, calculate the AH rxn for each of the following equations. Selected...
6-8 Using the table below, calculate the AH rxn for each of the following equations. Selected Standard Enthalpies of Formation at 25° C (298K) AH (kJ/mol) (kJ/mol Formula AH 0 Silver 92.3 Agis) AgC(3) 0 1270 218 Formula AH (kJ/mol Formula Calcium Ca(s) CI (9) Ca(s) 635.1 HC (G) Caco (s)-1206.9 Hydrogen Hig) Carbon C(graphite) 0 H (9) C(diamond) 1.9 Nitrogen COL) -1105 N19) CO(g) -393.5 NH,(g CH_(9) 74.9 NO(9) CH,OHI) -238.6 Oxygen HỎNG) 133 O.) CS.) 87.9 O (9)...
KINETICS AND EQUILIBRIUM Using an equilibrium constant to predict the direction of spont... A chemi... origineer...
KINETICS AND EQUILIBRIUM Using an equilibrium constant to predict the direction of spont... A chemi... origineer is studying the following reaction: 2NO(9)+2H,(0) N (9)+2H,0(9) At the temperature the engineer picks, the equilibrium constant for this reaction is 0.39. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions:...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions: (a) H(g)Cl(g) 2 HCl(g) (b) 2 C(s)+O2(g) 2 CO(g Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 O(g) 3 0:(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O, and 0.060 mol of NO2 at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant Ke for the reaction? N2O4(g) 2 NO:(g)...
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C....
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C. See Appendix C for data. Fe(s) + Cu2+ (aq) = Fe2+ (aq) + Cu(s) Find equilibrium constan + K at 25°C Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kJ/mol) AG; (kJ/mol (J/mol-K) 20.87 Substance or lon Ba(OH),(s) ΔΗ: (kJ/mol) -946.3 --3342.2 AG (kJ/mol) -859.3 -2793 (J/mol K) 107.1 427 Ba(OH), 8H,O(s) BaSO (8) - 1473.2 -1362.3 132.2...
help with these please N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables...
help with these please
N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: CH (9) +202(g) →CO2(g) + 2H2O(g) de manera en cas de este mai mare de mise en contact tenda Using standard thermodynamic data at 298K, calculate the free energy change when 1.62 moles of CH4(g) react at standard conditions. AGºrx Nz9) +202(g) +2NO2(g) Using standard thermodynamic data at 298K, calculate the free...
Using enthalpies of formation (Appendix C), calculate ΔH ° for the following reaction at 25°C. Also...
Using enthalpies of formation
(Appendix C), calculate ΔH ° for the following reaction at 25°C.
Also calculate ΔS ° for this reaction from standard entropies at
25°C. Use these values to calculate ΔG ° for the reaction at this
temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g).
Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got...
POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got Mol-aria Why? Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. This is called Stoichiometry- (stoi-key-ah-meh-tree) Another way of looking at it is using the mole ratio from the balanced equation and information about one compound in the reaction to determine information about another compound in the equation. A mole ratio...
#6-9 6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your...
#6-9
6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your book (Appendix 2): CH(g)+02(B) HO(g) + CO,(g) (not balanced) 7. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide: CaCO3 CO2+ CaO Using data from the textbook (Apendix 2), determine the heat of reaction. 8. When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCI+3 02 2KCIO3 Using data from the textbook (Appendix 2),...
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A, G, for various hstances at 298.15 K and one har 1057 Substance Formula 4,6°/kJ-mol- acetylene ammonia C.H,() NH,(g) CHCI) Br(e) CH) C(s) C(s) CO (8) CO(g) 209.20 - 16.367 124.35 3.126 -17.15 2.900 benzene bromine butane carbon(diamond) carbon(graphite) carbon dioxide carbon monoxide ethane ethanol ethene glucose hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen peroxide iodine methane methanol CH(E) сHOH(1) CH (8) CH...
eNaICUrate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,G", for various substances at 298.15 K and one bar. 1057 Substance Formula 4,G"/kJ-mol acetylene сН.0 NH,(g) ammonia 209.20 benzene -16.367 с,н.Ф 124.35 bromine Br (g) 3.126 butane C,Hog) -17.15 carbon(diamond) C(s) 2.900 carbon(graphite) C(s) carbon dioxide cO(g) -394.389 carbon monoxide COg) -137.163 ethane СН, С Н, ОнФ сН. Ф C,H,0,(s) HBr(g) НСK -32.82 ethanol -174.78 ethene 68.421 glucose -910.52 hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide -53.513...
6-8 Using the table below, calculate the AH rxn for each of the following equations. Selected Standard Enthalpies of Formation at 25° C (298K) AH (kJ/mol) (kJ/mol Formula AH 0 Silver 92.3 Agis) AgC(3) 0 1270 218 Formula AH (kJ/mol Formula Calcium Ca(s) CI (9) Ca(s) 635.1 HC (G) Caco (s)-1206.9 Hydrogen Hig) Carbon C(graphite) 0 H (9) C(diamond) 1.9 Nitrogen COL) -1105 N19) CO(g) -393.5 NH,(g CH_(9) 74.9 NO(9) CH,OHI) -238.6 Oxygen HỎNG) 133 O.) CS.) 87.9 O (9)...
KINETICS AND EQUILIBRIUM Using an equilibrium constant to predict the direction of spont... A chemi... origineer is studying the following reaction: 2NO(9)+2H,(0) N (9)+2H,0(9) At the temperature the engineer picks, the equilibrium constant for this reaction is 0.39. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions: (a) H(g)Cl(g) 2 HCl(g) (b) 2 C(s)+O2(g) 2 CO(g Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 O(g) 3 0:(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O, and 0.060 mol of NO2 at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant Ke for the reaction? N2O4(g) 2 NO:(g)...
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C. See Appendix C for data. Fe(s) + Cu2+ (aq) = Fe2+ (aq) + Cu(s) Find equilibrium constan + K at 25°C Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kJ/mol) AG; (kJ/mol (J/mol-K) 20.87 Substance or lon Ba(OH),(s) ΔΗ: (kJ/mol) -946.3 --3342.2 AG (kJ/mol) -859.3 -2793 (J/mol K) 107.1 427 Ba(OH), 8H,O(s) BaSO (8) - 1473.2 -1362.3 132.2...
help with these please
N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: CH (9) +202(g) →CO2(g) + 2H2O(g) de manera en cas de este mai mare de mise en contact tenda Using standard thermodynamic data at 298K, calculate the free energy change when 1.62 moles of CH4(g) react at standard conditions. AGºrx Nz9) +202(g) +2NO2(g) Using standard thermodynamic data at 298K, calculate the free...
Using enthalpies of formation
(Appendix C), calculate ΔH ° for the following reaction at 25°C.
Also calculate ΔS ° for this reaction from standard entropies at
25°C. Use these values to calculate ΔG ° for the reaction at this
temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g).
Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got Mol-aria Why? Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. This is called Stoichiometry- (stoi-key-ah-meh-tree) Another way of looking at it is using the mole ratio from the balanced equation and information about one compound in the reaction to determine information about another compound in the equation. A mole ratio...
#6-9
6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your book (Appendix 2): CH(g)+02(B) HO(g) + CO,(g) (not balanced) 7. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide: CaCO3 CO2+ CaO Using data from the textbook (Apendix 2), determine the heat of reaction. 8. When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCI+3 02 2KCIO3 Using data from the textbook (Appendix 2),...
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