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A student determines the value of the equilibrium constant to be 8.47x10-37 for the following reaction....
A student determines the value of the equilibrium constant to be 1.13x10 for the following reaction....
A student determines the value of the equilibrium constant to be 1.13x10 for the following reaction. 3Fe2O3(s) + H2(9)—2Fe3O4(s) + H20(9) Based on this value of Keg: AGº for this reaction is expected to be greater, less) than zero. Calculate the free energy change for the reaction of 1.52 moles of Fe,O3(s) at standard conditions at 298K. AGⓇxn = A student determines the value of the equilibrium constant to be 2.34x10-25 for the following reaction. CH (9) + H20(g)—+3H2(g) +...
A student determines the value of the equilibrium constant to be 6.51x109 for the following reaction....
A student determines the value of the equilibrium constant to be 6.51x109 for the following reaction. CO(g) + H2O(1) CO2(g) + H2(g) Based on this value of Keq: AGⓇ for this reaction is expected to be (greater, less) than zero Calculate the free energy change for the reaction of 2.00 moles of CO(g) at standard conditions at 298K. kJ AGºrxn
A student determines the value of the equilibrium constant to be 1.79x107 for the following reaction....
A student determines the value of the equilibrium constant to be 1.79x107 for the following reaction. Fe(s) +2HCI(aq)FeCl2(s) H2(g) Based on this value of Keg: ?Go for this reaction is expected to be greater, less) Calculate the free energy change for the reaction of 1.86 moles of Fe(s) at standard conditions at 298K than zero. kJ rxn
10. A student determines the value of the equilibrium constant to be 3.99x1013 for the following...
10.
A student determines the value of the equilibrium constant to be 3.99x1013 for the following reaction. 4HCK(g) + O2(g) +2H2O(g) + 2Cl2(g) Based on this value of Keq AGⓇ for this reaction is expected to be (greater, less) than zero Calculate the free energy change for the reaction of 2.45 moles of HCl(e) at standard conditions at 298K. AGºrx Submit Answer Retry Entire Group 9 more group attempts remaining A student determines the value of the equilibrium constant to...
A student determines the value of the equilibrium constant to be 6.99×104 for the following reaction....
A student determines the value of the equilibrium constant to be 6.99×104 for the following reaction. S(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite) Based on this value of Keq: G° for this reaction is expected to be (greater, less) than zero. ________ Calculate the free energy change for the reaction of 1.74 moles of S(s,rhombic) at standard conditions at 298K. G°rxn = kJ
A student determines the value of the equilibrium constant to be 2.58×10-25 for the following reaction....
A student determines the value of the equilibrium constant to be 2.58×10-25 for the following reaction. CH4(g) + H2O(g)---->3H2(g) + CO(g) Based on this value of Keq: Delta G° for this reaction is expected to be (greater, less)?____ than zero. Calculate the free energy change for the reaction of 2.33 moles of CH4(g) at standard conditions at 298K. DeltaG°rxn =____? kJ
A student determines the value of the equilibrium constant to be 2.38*10-10 for the following reaction....
A student determines the value of the equilibrium constant to be 2.38*10-10 for the following reaction. Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O(g) Based on this value of Key AGⓇ for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 2.20 moles of F,036) at standard conditions at 298K. kJ than zero. AG Submit Answer Retry Entire Group 9 more group attempts remaining
A student determines the value of the equilibrium constant to be 1.5297 x 107 for the...
A student determines the value of the equilibrium constant to be 1.5297 x 107 for the following reaction: HBr(g) + 1/2 Cl2(g) --> HCl(g) +1/2 Br2(g) Based on this value of Keq, calculate the Gibbs free energy change for the reaction of 2.37 moles of HBr(g) at standard conditions at 298 K. Group of answer choices ΔGº = +97.1 kJ ΔGº = -82.0 kJ ΔGº = +194.2 kJ ΔGº = -97.1 kJ ΔGº = -194.2 kJ How long would it...
inneed help please! thanks QUESTION 31 (5 marks) The equilibrium constant at 37°C for the reaction...
inneed help please! thanks
QUESTION 31 (5 marks) The equilibrium constant at 37°C for the reaction cisaconitate isocitrate 2.5. reaction mixture is prepared with isocitrate at a concentration of 0.2 M, and cisaconitate at a concentration of 0.001 M. Which species is favoured (present in greater amount) when the system is at equilibrium? fraducts Calculate the free energy change for this reaction under these conditions. G RT E -3 x 10 x 2 . C .31 XiD G 20-1 Answer...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
A student determines the value of the equilibrium constant to be 1.13x10 for the following reaction. 3Fe2O3(s) + H2(9)—2Fe3O4(s) + H20(9) Based on this value of Keg: AGº for this reaction is expected to be greater, less) than zero. Calculate the free energy change for the reaction of 1.52 moles of Fe,O3(s) at standard conditions at 298K. AGⓇxn = A student determines the value of the equilibrium constant to be 2.34x10-25 for the following reaction. CH (9) + H20(g)—+3H2(g) +...
A student determines the value of the equilibrium constant to be 6.51x109 for the following reaction. CO(g) + H2O(1) CO2(g) + H2(g) Based on this value of Keq: AGⓇ for this reaction is expected to be (greater, less) than zero Calculate the free energy change for the reaction of 2.00 moles of CO(g) at standard conditions at 298K. kJ AGºrxn
A student determines the value of the equilibrium constant to be 1.79x107 for the following reaction. Fe(s) +2HCI(aq)FeCl2(s) H2(g) Based on this value of Keg: ?Go for this reaction is expected to be greater, less) Calculate the free energy change for the reaction of 1.86 moles of Fe(s) at standard conditions at 298K than zero. kJ rxn
10.
A student determines the value of the equilibrium constant to be 3.99x1013 for the following reaction. 4HCK(g) + O2(g) +2H2O(g) + 2Cl2(g) Based on this value of Keq AGⓇ for this reaction is expected to be (greater, less) than zero Calculate the free energy change for the reaction of 2.45 moles of HCl(e) at standard conditions at 298K. AGºrx Submit Answer Retry Entire Group 9 more group attempts remaining A student determines the value of the equilibrium constant to...
A student determines the value of the equilibrium constant to be 2.38*10-10 for the following reaction. Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O(g) Based on this value of Key AGⓇ for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 2.20 moles of F,036) at standard conditions at 298K. kJ than zero. AG Submit Answer Retry Entire Group 9 more group attempts remaining
inneed help please! thanks
QUESTION 31 (5 marks) The equilibrium constant at 37°C for the reaction cisaconitate isocitrate 2.5. reaction mixture is prepared with isocitrate at a concentration of 0.2 M, and cisaconitate at a concentration of 0.001 M. Which species is favoured (present in greater amount) when the system is at equilibrium? fraducts Calculate the free energy change for this reaction under these conditions. G RT E -3 x 10 x 2 . C .31 XiD G 20-1 Answer...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
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