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(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.)...
1. From the following equations and enthalpies, determine the molar heat of formation of HNO2(aq) . NH4NO2(aq) → N2(g) + 2H2O(l) ∆H = -320.1 kJ NH3(aq) + HNO2(aq) → NH4NO2(aq) ∆H = -37.7 kJ 2NH3(aq) → N2(g) + 3H2(g) ∆H = +169.9 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆H = -285.8 kJ
Appropriately combine the measured enthalpies of reactions (2) and (3) to predict (delta)H1 for the following reaction: Reaction (1): CaCO3(s) + H2O(l) ------> Ca(OH)2 (g) + CO2 (g) (delta) H1 equals what? Based on the predicted enthalpy, indicate whether Reaction (1) is endothermic or exothermic. Reaction (1) CaCO3(s) + H2O(l) ----> Ca(OH)2(s) + CO2(g) Reaction (2) CaCO3(s) + 2HCl (aq) ----> CaCl2(aq) + H2O(l) + CO2(aq) Reaction (3) CaCl2(aq) + 2H2O(l) ----> Ca(OH)2(s) + 2HCl(aq)
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Select the Redox Reactions: A) Mg + 2H+--> Mg2+ +H2(g) B) K2CO3(aq) + Sr(NO3)2(aq)--> SrCO3(s) + 2KNO3(aq) C) 2OH- + 2ClO-2 --> ClO2- + ClO3- + H2O D) H+ + OH- --> H2O E) KSCN (aq) + Fe(NO3)3(aq) --> FeSCN2+(aq) + KNO3 (aq) + 2NO3- (aq) F) AgCl(s) +2NH3(aq) --> Ag(NH3)2+ (aq) +Cl- (aq)
Part A Several reactions and their standard reaction enthalpies at 298.15 K are given here: Al_C3(s) + 12H2O(l) + 4Al(OH),(s) + 3CH4(g) 2Al(s) + O2(g) + Al2O3(s) 1 A1,03(s) + H2O(l) + Al(OH)3(s) AH (kJ. mol-?) –1683.0 -1675.7 -9.6 The standard enthalpies of combustion of graphite and CH4(8) are -393.51 and --890.35 kJ. molº respectively. Calculate the standard enthalpy of formation of Al4C3(s) at 25°C.
Question 4 of 4 > The enthalpy changes, AH, for three reactions are given. H, ()0,()H,O) Ca(s) +2H (aq) Ca2 (aq) +H,(g) CaO(s) +2H (aq) - AH=-286 kJ/mol AH= -544 kJ/mol Ca2 (aq) +H,O() AH =-193 kJ/mol Using Hess's law, calculate the heat of formation for CaO(s) using the reaction shown. 0,()Ca) Ca(s) + kJ/mol ΔΗ- TOOLS During an experiment, a student adds 1.81 g CaO to 300.0 mL of 1.000 M HCI. The student observès a temperature increase of...
a. Determine the Molar Enthalpies for the two reactions listed below. In each case, an excess of HCI is Temp. 2. Calorimetry used as the reactant. You can assume that the reactants are dilute within the aqueous system. Reaction Total Mass of Mass of Al (g) AlbOs (g) volume of change water (ml I-cc) +9.3 100 100 Al 0,(s)t lici (aq)-> 2.AP. (aa) -31 100g)一しNUA-しー0.3 b. Using calculations from, part a and the information provided below, determine ΔΗ' for the...
Part A Several reactions and their standard reaction enthalpies at 298.15 K are given here: AH (kJ · mol-?) CaC2 (s) + 2H2O(1) + Ca(OH)2 (s) + C2H2 (g) –127.9 Ca(s) + O2(g) → Cao(s) CaO(s) +H2O(1) + Ca(OH)2(s) -65.2 -635.1 The standard enthalpies of combustion of graphite and C2H2(g) are –393.51 and — 1299.58 kJ · mol-? respectively. Calculate the standard enthalpy of formation of CaC2(s) at 25°C. Express your answer to one decimal place and include the appropriate...
Classify the half‑reactions as reduction half‑reactions or oxidation half‑reactions. H2(g)⟶2H+(aq)+2e−H2(g)⟶2H+(aq)+2e− 12O2(g)+2H+(aq)+2e−⟶H2O(g)12O2(g)+2H+(aq)+2e−⟶H2O(g) Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e− 2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq)2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq) Fe(s)⟶Fe2+(aq)+2e−Fe(s)⟶Fe2+(aq)+2e− oxidation reduction reduction oxidation reduction