3. (6 points) Consider the reaction: H2 (g) + Br2 (g) = 2HBr (g), where AH...
Consider the reaction 2HBr(g) H2(g) Br2(1) The standard free energy change for this reaction is 107.0 kJ. The free energy change when 2.50 moles of HBr(g) react at standard condition is kJ. What is the maximum amount of useful work that the reaction of 2.50 moles of HBr(g) is capable of producing in the surroundings under standard conditions? If no work can be done, enter none. kJ
Consider the reaction 2HBr(g) H2(g) Br2(1) The standard free energy change for this...
Consider the reaction: 2HBR(g) >H2(g) + Br2() Using standard thermodynamic data at 298K, calculate the free energy change when 1.51 moles of HBr(g) react at standard conditions AG° kJ rxn AHof (kJ/mol) AG°F (kJ/mol) s° (J/mol K) Beryllium Вe(s) 0 9.5 -569.0 ВeO(s) -599.0 14.0 Be(ОН)2(s) -902.5 -815.0 51.9 AH°f (kJ/mol) AG°f (kJ/mol) s° (J/mol K) Bromine Br(g) 111.9 175.0 82.4 Br2() 152.2 0 0 Br2(g) 30.9 3.1 245.5 Br2(aq) -3.0 4.0 130.0 -121.0 -175.0 82.0 Br (aq) BrF3(g) -255.6...
What is AG at 298 K for the following reaction? H2(g) + Brz(9) -2HBr(g): AH = -103.8 kJ; AS = 21.3 J/K at 298 K -110.1 kJ 6.451 * 10 kJ 97.45 kJ -6.451 x 10'
10. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 13.7−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] = [Br2] = [HBr] =
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 1.20 moles of HBr in a 21.3−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.
2-Consider the reaction H2(g) + Br2(g) 2 HBr (g⇌ ) where ΔHo = -36.4 kJ/mol. In one experiment, equal amounts in moles of H2(g) and Br2(g) were mixed in a 2.00 L chamber at 25 oC exerting a pressure P = 1.0 atm. After mixture reached equilibrium, partial pressure of H2 gas PH2 was measured using high sensitivity HVAC gauge recording, PH2 = 5x10-4 Pa. For this equilibrium reaction, answer the following: (i)Calculate the total amount nT of gases...
Consider the reaction: 2HBr(g)H2(g) + Br2(l) Using standard thermodynamic data at 298K, calculate the free energy change when 2.33 moles of HBr(g) react at standard conditions. G°rxn = _____kJ
At 1000 K, Kp=2.1×106 and ΔH∘ = -101.7 kJ for the reaction H2(g)+Br2(g)⇌2HBr(g). A 0.950 mol quantity of Br2 is added to a 1.00 L reaction vessel that contains 1.24 mol of H2 gas at 1000 K. What are the partial pressures of H2, Br2, and HBr at equilibrium?
Consider the reaction: 2HBr(g)—„H2(g) + Br26) Using standard thermodynamic data at 298K, calculate the free energy change when 1.84 moles of HBr(g) react at standard conditions. AG°rxn= C kJ
The Kc of the reaction H2 (g)+Br2 (g)=2HBr (g) is 2.18×10+6. If the initial concentration of HBr in 12.0L vessel is 3.20 moles, calculate the concentration of H2, Br2 and HBr at equilibrium. Use ICE table. Show calculations and all work & may have to use quadratic equation.