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- C2H5OH = delta H = -278 KJ/mol, delta G = -175 KJ/mol, S = 161 J/K mol 3O2 = delta H = 0 KJ/mol, delta G = 0 KJ/mol, S = 205.152 J/K mol 2Co2 = delta H = -393.5 KJ/mol, delta G = -394 KJ/mol, S = 214 J/K mol 3H2O = delta H = -242 KJ/mol, delta G = -229 KJ/mol, S = 189 J/K molCalculate ΔH°rxn using the following information: SO2I2(g) + 2 H2O(l) → 2 HI(g) + H2SO4(l) ΔH°rxn = ? ΔH°f (kJ/mol) SO2I2(g) -264 H2O(l) -286 HI(g) -12 H2SO4(l) -814The ΔH°f for H2O(g) is -241.8kJ/mol. Find the ΔH°rxn (in kJ/mol) of 2H2O(g) → 2H2(g) + O2(g) Choices: A. 483.6 B. -241.8 C. 241.8 D. -483.6
- 1. Find ∆Hf for Al2O3 using the following data 2 Al + 3/2 O2 ----> Al2O3 H2 + ½ O2 ------------> H2O ∆H1 = –286 kJ/mol 2 Al + 6 H+ -------------> 2 Al3+ + 3 H2 ∆H2 = –1050 kJ/mol Al2O3 + 6 H+ -----------> 2 Al3+ + 3 H2O ∆H3 = –238 kJ/mol NOTE: I calculated #5 to be ∆Hf =-1670 kJ/mol. 6. Using the value calculated in #5, find the temperature change expected when 0.100 g Al reacts with oxygen if the calorimeter used has a heat capacity of 420 J/°C.True or false Kc= [NH3]2 /[N2]2[H2]3 for N2+3H2<--> 2NH3MW is 98 1HNMR: 1.7 quintet, 1.8 quintet, 2.3 triplet What molecule is this?
- HOCI HF HCN H₂SO4 HOBr 2.29 x 10-8 O 2.30 K₂= 3.510-8 O 1.17 x 108 O 1.45 x 10-7 K₂ = 7.2 10-4 K₂ = 4.010-10 K₁ = very large K₂ = 1.2 10-2 Ka = 2.5210-⁹ (COOH)2 CH3COOH C6H5NH2 NH3 K₁ = 5.9 x 10-² K₂ = 6.4 x 10-5 K₂ = 1.8 x 10-5 Refer to Equilibrium Constants. What is the [H3O+] of a solution that is 0.0100 M in HOCland 0.0300 M in NaOCI? Kb = 4.2 x 10-10 Kb = 1.8 x 10-5Calculate Delta Hof for PbO (s) using the data below. PbO (s) + CO (g) ® Pb (s) + CO2 (g) DH° = –131.4 kJ DHf°: CO2(g) = –393.5 kJ/mol; CO(g) = –110.5 kJ/mol –151.6 kJ/mol –283.0 kJ/mol +283.0 kJ/mol –372.6 kJ/mol +252.1 kJ/molComplete the equation, using appropiate notations and fromulas: 410Be=?+510B