Question 41 of 50 Submit Using the provided table, determine the enthalpy for the reaction 2...
Question 14 of 20 Submit Using the provided table, determine the enthalpy for the reaction 2 K(s) + 2 H2O(l) → 2 KOH (aq) + H2(g) Substance AH1° (kJ/mol K(s) 0 H2O (1) -285.8 KOH (aq) -482.4 H2 (g)
Question 14 of 14 Submit Using the provided table, determine the enthalpy for the reaction 2 NHs (g) 3 N2O (g) - 4 N2 (g) +3 H2O (I) Днғ (kJ/mo) Substance NH3 (g) -46.2 N2O (g) 81.6 N2 (g) 0 НаО () -285.8 kJ/mol х 1 2 4 5 6 с 7 8 +- 0 x 100 Tap here or pull up for additional resources 32
Question 42 of 50 Submit Using the provided table, determine the enthalpy for the reaction C(s) + CO2(g) – 2 CO (9) Substance AH (kJ/mol) C (s) 0 CO2 (g) -393.5 kJ/mol 1 2 3 C +/- : 0 x 100
Question 14 0414 Using the provided table, determine the enthalpy for the reaction 2 NH3 (g) + 3 N20 (g) - 4 N2 (g) + 3 H20 (1) Substance AHI (kJ/mol) NH3(g) -46.2 N20 (9) 81.6 N2 (9) 0 kJ/mol
Question 43 of 50 Submit Using the provided table, determine the enthalpy for the reaction 2 NH3(g) + 3 N20 (g) - 4 N2 (9) + 3 H2O (1) Substance AH (kJ/mol) NH3 (9) -46.2 N20 (g) 81.6 N2 (9) kJ/mol 1 2 3 C +/- : 0 x 100
Using the provided table and the equation below, determine the heat of formation for KCIO2. 2 KCIO: (s) 2 KCIO2 (s) + O2 (g) AH° = 296.2 kJ/mol Substance kJ/mol AHi" (kJ/mol) KCIO3 (s) -391.2 1 3 2 4 5 6 с O2 (g) 0 7 8 9 +/- 0 X 100
Question 16 of 20 Submit Using the provided table, determine the enthalpy for the reaction C3H2 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AHF (kJ/mol) C3H8 (9) -108.4 O2 (9) CO2 (g) -393.5 H2O (9) -241.8
2. Lastly, use the table of thermodynamic functions to compute the AHo and ASo for the reactions in #1. Then using AH° and AS° and your knowledge of the second law, compute which reactions are spontaneous under standard conditions. You must show all your calcualtions. (7pts) Spontaneous ASo ASuniv ΔΗ Reaction 2H2(g) + 02(g) 2H20() CO2(s)-CO2(g) K (aq)+ Cl (aq)- KCI(s) Thermodynamic Properties at 298 K AH AG Substance kJ/mol kJ/mol 3/(mol-K) Ag(s) Ag (aq) AgBr(s) AgCls) Agl(s) Cl:(g) CI(8)...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
Question 36 of 50 Submit Using the equations N2(g) + 3 H2(g) - 2 NH; (g) AH = -91.8 kJ/mol C(s) + 2 H (g) – CH2 (g) AH° = -74.9 kJ/mol H2 (g) + 2c(s) + N2 (g) - 2 HCN (g) AH = 270.3 kJ/mol Determine the enthalpy for the reaction CH, (g) + NH4 () – HCN (g) + 3 H2(g). kJ/mol 1 2 3 C +/- : 0 x 100