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Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the...
Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(a...
Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 90.3 86.6 210.8 NO(9) NOCI(g) 51.7 66.1 261.8 NO2(g) 33.2 51.3 240.1 N20(9) 82.1 104.2 219.9 N204(9) 9.2 97.9 304.3 N204(0) -20.0 97.0 209.0 N205(s) -42.0 134.0 178.0 N2H4(0) 50.6 149.3 121.2 N2H3CH3 () 54.0 180.0 166.0 HNO3(aq) -207.4 -111.3 146.4 HNO3(1) -174.1 -80.7 155.6 HNO3(9) -135.1 -74.7 266.4 NH4ClO4(s) -295.0...
Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) N2 (g) 0 0 191.6 472.7 455.6 153.3...
Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) N2 (g) 0 0 191.6 472.7 455.6 153.3 N(g) NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO (g) 90.3 86.6 210.8 NOCI (g) 51.7 66.1 261.8 NO2 (g) 33.2 51.3 240.1 N20 (g) 82.1 104.2 219.9 N204 (8) 9.2 97.9 304.3 Consider the reaction N2(9) + 202(9)—2NO2(g) Using the standard thermodynamic data in the tables linked above, calculate Grxn for this reaction at 298.15K...
help with these please N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables...
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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...
help with this please Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic...
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Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: 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: 2CO(g) + O2(g) +2002(9) - der e en manos de 20, ali ne more than one so mi dicogna undan Using standard thermodynamic data...
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol...
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol K) 0 205.1 Oxygen 02 (g) O(g) 03 (g) 249.2 231.7 161.1 142.7 163.2 238.9 Phosphorus AH° (kJ/mol) AG°f(kJ/mol) sº (/mol K) Nitrogen AH°(kJ/mol) AG°f(kJ/mol) s° /mol K) N2 (8) 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 132.0 -79.0 113.0 90.3 86.6 210.8 51.7 66.1 261.8 NH4+ (aq) NO (g) NOCI (9) NO2 (g)...
Use the data from this table of thermodynamic properties to calculate the values of ASixn for...
Use the data from this table of thermodynamic properties to calculate the values of ASixn for each reaction at 25 °C. 4NH,(g) + 70,(9) — 4NO2(g) + 6H2O(g) AS:n = J/mol K N,() + 0,(g) 2 NO(g) J/mol K Asian = MISU415) -1065.25 N2(9) N2H4(0) 50.6 N20(9) 81.6 N204(9) 11.1 N205(9) 13.3 NH3(9) -45.9 NH3(aq) -80.29 NH,+(aq) -133.3 NH4CI(S) -314.4 NH4NO3(s) -365.6 (NH2)2CO(s) -333.1 Na(s) Na+(aq) -240.3 Na2CO3(S) -1130.7 NaCl(s) -411.2 NaF(s) -576.6 NaBr(s) -361.1 Nal(s) -287.8 NaNO3(s) -467.9 NaOH(s)...
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy...
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the...
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 14.96 mm Hg. 2N2(g) + O2(g)2N2O(g) G =_____ kJ/mol
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for...
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for : Mark 1.00 out of 1.00 2002(g) +4H2O(1) ► 2CH3OH(1) + 302(g) P Flag question Answer: 1404.84 Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AGⓇ =AH°-TAS and assume AH° and AS are independent of temperature. P Flag question (Theis...
Calculate the AG" value at 500 K for the reaction given below. Is the reaction voluntary...
Calculate the AG" value at 500 K for the reaction given below. Is the reaction voluntary under conditions where the pressure of each H2 (g) and H20 (g) gas is 1 atm each? Cu (S) + H20 (g) → CuO (S) + H2 (g) 500K AHºf (kJ/mol) Sº (J/mol K) Cu (S). 0 33.3 H2O (g.hu -241.8 188.7 CuO (S) -155.2 43.51 H2 (g) 0 130.6
Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 90.3 86.6 210.8 NO(9) NOCI(g) 51.7 66.1 261.8 NO2(g) 33.2 51.3 240.1 N20(9) 82.1 104.2 219.9 N204(9) 9.2 97.9 304.3 N204(0) -20.0 97.0 209.0 N205(s) -42.0 134.0 178.0 N2H4(0) 50.6 149.3 121.2 N2H3CH3 () 54.0 180.0 166.0 HNO3(aq) -207.4 -111.3 146.4 HNO3(1) -174.1 -80.7 155.6 HNO3(9) -135.1 -74.7 266.4 NH4ClO4(s) -295.0...
Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) N2 (g) 0 0 191.6 472.7 455.6 153.3 N(g) NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO (g) 90.3 86.6 210.8 NOCI (g) 51.7 66.1 261.8 NO2 (g) 33.2 51.3 240.1 N20 (g) 82.1 104.2 219.9 N204 (8) 9.2 97.9 304.3 Consider the reaction N2(9) + 202(9)—2NO2(g) Using the standard thermodynamic data in the tables linked above, calculate Grxn for this reaction at 298.15K...
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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...
help with this please
Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: 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: 2CO(g) + O2(g) +2002(9) - der e en manos de 20, ali ne more than one so mi dicogna undan Using standard thermodynamic data...
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol K) 0 205.1 Oxygen 02 (g) O(g) 03 (g) 249.2 231.7 161.1 142.7 163.2 238.9 Phosphorus AH° (kJ/mol) AG°f(kJ/mol) sº (/mol K) Nitrogen AH°(kJ/mol) AG°f(kJ/mol) s° /mol K) N2 (8) 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 132.0 -79.0 113.0 90.3 86.6 210.8 51.7 66.1 261.8 NH4+ (aq) NO (g) NOCI (9) NO2 (g)...
Use the data from this table of thermodynamic properties to calculate the values of ASixn for each reaction at 25 °C. 4NH,(g) + 70,(9) — 4NO2(g) + 6H2O(g) AS:n = J/mol K N,() + 0,(g) 2 NO(g) J/mol K Asian = MISU415) -1065.25 N2(9) N2H4(0) 50.6 N20(9) 81.6 N204(9) 11.1 N205(9) 13.3 NH3(9) -45.9 NH3(aq) -80.29 NH,+(aq) -133.3 NH4CI(S) -314.4 NH4NO3(s) -365.6 (NH2)2CO(s) -333.1 Na(s) Na+(aq) -240.3 Na2CO3(S) -1130.7 NaCl(s) -411.2 NaF(s) -576.6 NaBr(s) -361.1 Nal(s) -287.8 NaNO3(s) -467.9 NaOH(s)...
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for : Mark 1.00 out of 1.00 2002(g) +4H2O(1) ► 2CH3OH(1) + 302(g) P Flag question Answer: 1404.84 Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AGⓇ =AH°-TAS and assume AH° and AS are independent of temperature. P Flag question (Theis...
Calculate the AG" value at 500 K for the reaction given below. Is the reaction voluntary under conditions where the pressure of each H2 (g) and H20 (g) gas is 1 atm each? Cu (S) + H20 (g) → CuO (S) + H2 (g) 500K AHºf (kJ/mol) Sº (J/mol K) Cu (S). 0 33.3 H2O (g.hu -241.8 188.7 CuO (S) -155.2 43.51 H2 (g) 0 130.6
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