Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX: \longrightarrow ⟶ 7 N2(g) + 12 H2O(l) LaTeX: \Delta Δ G°rxn = ? LaTeX: \Delta Δ G°f (kJ/mol) –73.5 149.3 –237.1
Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX:...
Calculate ΔGorxn given the following information. 4HNO3(g) + 5N2H4(l) → 7N2(g) + 12H2O(l) HNO3(g) N2H4(l) N2(g) H2O(l) ΔGof (kJ/mol) -73.5 149.3 0 -237.1
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0 -151 kJ +50.8 kJ -186 kJ +222 kJ -85.5 kJ
Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0
Question 7 0.5 pts Determine the sign of ASsur and ASsys for the following chemical reaction at 298 K: C3H8 (8)+5 O2 (g)3 CO2(g)+4 H20(g)AH nxn-2044 k Question 8 0.5 pts Calculate the ?Gnn for the following reaction. 4 HNOg(g) + 5 N2H4(1)-7 N2(g) + 12 H2on HNO3(g) N2H4l) H20() G"f (kJ/mol) 73.5 149.3 237.1 O-3.886x103 kJ 0-3298x103 ? -2.393x103kJ 3.298 kJ + 3298x103 kJ
Given the following data: (1) 2 H2(g) + CO2(g) LaTeX: \longrightarrow ⟶ CH4(g) + O2(g) DGorxn = 343 KJ (2) 2 H2(g) + O2(g) LaTeX: \longrightarrow ⟶ 2 H2O(l) DGorxn = -474 KJ Calculate DGorxn (kJ) for (3) CH4(g) + 3 O2(g) + 2 H2(g) LaTeX: \longrightarrow ⟶ CO2(g) + 4 H2O(l) DGorxn = ??? Only enter a numerical value.
calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187.8 kJ
Determine delta G(not) rxn using the following information. Assume standard cognitions. 2H2S(g) +3O2(g) --> 2H2O(l)+2SO2(g) Delta H (not): 1.12 kJ Delta S(not): -390.7 J/K
Calculate the standard entropy, Δ?∘rxn, of the reaction at 25.0 ∘C using the table of thermodynamic properties. 3C2H2(g)⟶C6H6(l) Δ?∘rxn= J⋅K−1⋅mol−1 Calculate the standard Gibbs free energy of the reaction, Δ?∘rxn. The standard enthalpy of the reaction, Δ?∘rxn, is −633.1 kJ⋅mol−1. Δ?∘rxn= kJ⋅mol−1 Determine in which direction the reaction is spontaneous as written at 25.0 ∘C and standard pressure. both forward reverse neither
Calculate
rxn for the below combustion reaction, determine if
entropy increases or decreases. Assume 1 mol of substance at 25
Celsius.
C3H8(g) + 5O2(g)
3CO2(g) + 4H2O(l)
Delta G of C3H8 = -23.4 kj/mol
Delta G of O2 = 0 kj/mol
Delta G of CO2 = -394.36 kj/mol
Delta G of H2O = -237.1 kj/mol
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