1. A mixture of 3.00 mol of Cl2 and 3.00 mol of H20 are enclosed in...
A mixture of 3.00 mol of Cl2 and 3.00 mol of CO is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2(g) = COCl2(g) Calculate Kc for the reaction at 600.°C. Calculate deltaG for the reaction at this temperature. = kJ/mol CO(g)= deltaH= -110.5 (kJ/mol) deltaG= -137.2 (kj/mol) S= 197.7 (j/molK) Cl2(g)= S= 223.1 J/molK COCl2(g)= deltaH= -218.8(kJ/mol) deltaG= -204.6 (kj/mol) S= 197.7 J/molK
I don't get how to do 5 or or co2, 0.750 mol of H20, and 1.00 mol of CO to a 5.00 L reactor at 990 CO2 (g) + H2 (g) H2O (g) + CO (g) 5. At 35°C, the equilibrium constant (Kc) for the reaction below is 1.6x 10. An equilibrium mixture was found to have the following concentrations of Cl2 and NOCI: [Cl2] = 1.2 x 10-2 M; [NOCl] = 2.8 × 10-1 M. Calculate the concentration of...
A mixture of 0.008603 mol of Cl2, 0.05744 mol of H2O, 0.05353 mol of HCl, and 0.06453 mol of O2 is placed in a 1.0-L steel pressure vessel at 1529 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.006795 mol of Cl2 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. Peq(Cl2) = . Peq(H2O) = . Peq(HCl) = . Peq(O2) = . (b) Calculate...
A mixture of 0.1468 mol of Cl2, 0.04712 mol of H2O, 0.02609 mol of HCl, and 0.1672 mol of O2 is placed in a 1.0-L steel pressure vessel at 579 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.006984 mol of HCl is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. Peq(Cl2) = ? Peq(H2O) = ? Peq(HCl) = ? Peq(O2)...
A mixture of 0.482 M H20, 0.419 M Cl20, and 0.748 M HCIO are enclosed in a vessel at 25 °C. (Reaction) H2O(g) + C12O (g) <------> 2HOCI(g) Kc = 0.090 at 25 °C Calculate the equilibrium concentrations of each gas at 25 °C [H2O] = M [Cl2O] = M [HOCL]= M
5-7 (ACS-style) A mixture of 2.0 mol of CO (g) and 2.0 mol of H20 (g) was allowed to come to equilibrium in a 10.0-L flask at a high temperature. If Kc = 4.0, what is the molar concentration of H2 (g) in the equilibrium mixture? The equation for the reaction is: CO(g) + H20 (g) 5 CO2(g) + H2 (g) A) 0.67 M B) 0.40 M C) 0.20 M D) 0.13 M
I NEED A COMPLETE AND CLEAR SOLUTION PLEASE! thanks A mixture of 0.10 mol of NO, 0.050 mol of H2 and 0.10 mol of H2O is placed in a 1.0-L flask and allowed to reach equilibrium as shown below: 2 NO (g) +2 H(g)N2 (g) + 2 H2O (g) At equilibrium [NO] = 0.062 M. Calculate the equilibrium constants Kc and Kp for this reaction.
Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K The reaction is allowed to reach equilibrium in a 15.2-L flask. At equilibrium, [PCIs]-9.75x102 M, [PCl,]-o.156 M and [C12] = 0.156 M. (a) The equilibrium mixture is transferred to a 7.60-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 7.60-L flask. [PCI5] [C12] =
A mixture of 0.5540 M CO and 0.3180 M Cl2 is enclosed in a vessel and heated to 1000 K. cog) +Cl2(g) 근 COC12(g) Kc =255.0 at 1000 K Calculate the equilibrium concentration of each gas at 1000 K. Number Number Number
A mixture of 0.1148 mol of O2, 0.03185 mol of NOCI, 0.1467 mol of NO2, and 0.2587 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 436 K. The following equilibrium is established: 102(9) + 2 NOCI(9) = 2 NO2(g) + 1 C12(9) At equilibrium 0.008912 mol of NOCI is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of O2, NOCI, NO, and Cl2. Peq(O2) = x . Pea(NOCI) = Peg(NO2) = x ....