A +4B --> C+4D AHxn = ? Solve for AHrxn using the following reactions: E +...
Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔH = -461.7 kJ mol-1 E + F → C + 2D ; ΔH = 279.9 kJ mol-1 ½ E + G → H ; ΔH = -203.2 kJ mol-1 Calculate ΔH for the following reaction (in kJ mol-1) using Hess's Law: A + B + 4G +4D → 4H + 2F
11) Given the following reactions A+FC+2D 2E+F2D E+FB AH=-622.3 kJ AH = -285.8 kJ AH=-187.8 kJ the enthalpy of the reaction A + 2B C+ 4D iskJ.
. (14 pts) Using the reactions in the data section, calculate AHrxn for the reaction 8 Ni(s) S&(s) +12 O2(g)8 NiSOs(s) Data: NiSos() >NiO(s)+ SO2(g) 1/4 S8(s) + 202(g) >2 SO2(g) Ni(s) + ½ O2(g) > NiO(s) AHm" = 156 kJ/mole ,no=-594 kJ/mole AHn 241 kJ/mole rxn
Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔH =-228.3 kJ mol-1 C +2D E+F AH 493.9 kJ mol -1 E + G → H ; ΔH = 314.3 kJ mor! Calculate ΔΗ for the following reaction (in kJ mol-1) using Hess's Law: A B4D+4G-4H+2F
Calculate the change in enthalpy (in kJ) for the following theoretical reaction equation: A + 2B => 4C ΔH = ? Use the following information: 2D => A ΔH = +85 kJ 2C => B + D ΔH = -16 kJ B + 2D => 2E ΔH = +27 kJ ______________________________________________ Calculate the change in enthalpy (in kJ) for the following theoretical reaction equation: A + B => C + 3D ΔH = ? Use the following information: 3D +...
A. 5.84 B. 4.94 C. 0.392 D. 1.51 E. 0.281 1. Use the following reactions and their equilibrium constants to predict the equilibrium constant for this reaction: 2A(aq)+B(aq)3D(g) Kc-??? 4F(ag) 2A(aq) Kc-0.332 1/4B(ag)+F(aq) 3/4D(g)
carbon. Determine the AHrxn for C (diamond) → C (graphite), using the following thermochemical equations: a) C (diamond) + 02 (9) → CO2 (9) AH = -395.4 kJ b) CO (9) + 12 02 (9) → CO2 (9) AH = -283.0 kJ c) C (graphite) + CO2 (9) ► 2 CO (9) AH = +172.5 kJ
la b c Given that d e f =-1 , find 18 hill | 2a 2b 2c -2d -2e | 6g 6h 6i || 2a 2b 2c | |-20 -2e -2f= | 6g 6h 6i exact number, no tolerance
13) Calculate &G. for the following reactions at 25°C by using the given ΔG: (a) Nİg) + Ols)-> 2NO(g), (b) H0() H:0(g), and (c) 2C2H(8)+50(8)4CO (8)+2H:O(U) &Gr(NO)-86.7 kJ/mol, aGo[H,0(I)]s-237.2 k/mol, aGe[H2O(g))--228.6 kJ/mol;
Given the following enthalpy change values for the reactions below: A + 2B → C ; ΔrH = 136.5 kJ mol-1 2C + D → E + F ; ΔrH = -319.8 kJ mol-1 ½ E → G + 2B ; ΔrH = -296.9 kJ mol-1 Calculate ΔrH for the following reaction (in kJ mol-1) using Hess's Law: 2A + D → F + 2G