Given
H3AsO4(aq) + 4H2(g) → AsH3(g) + 4H2O(l)
ΔHf [AsH3(g)] = 66.4 kJ/mol
ΔHf [H3AsO4(aq)] = -904.6 kJ/mol
ΔHf [H2O(l)] = -285.8 kJ/mol
ΔHf [H2 (g)] = 0 kJ/mol
Now
ΔH°rxn = (∑ΔHf(products)) - (∑ΔHf(reactants))
=( ΔHf [AsH3(g)]+ 4*ΔHf [H2O(l)]) - (ΔHf [H3AsO4(aq)]+ 4*ΔHf [H2])
= (66.4 kJ/mol+4*-285.8 kJ/mol) – (-904.6 kJ/mol+0)
= -1076.8 kJ/mol + 904.6 kJ/mol
= -172.2 kJ/mol
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Given
2Fe(s) + O2(g) --> 2 FeO(s) ΔH=-544.0 kJ ------------------(1)
4Fe(s) + 3O2(g) --> 2 Fe2O3(s) ΔH= -1648.4 kJ------------------(2)
Fe3O4(s) --> 3Fe(s) + 2O2(g) ΔH= +1118.4 kJ------------------(3)
Now
reverse (1) and divide by
FeO(s) --> Fe(s) + 1/2O2(g) ΔH = 544.0/2 kJ --------------(4)
reverse (2) and divide by 2
Fe2O3(s) --> 2Fe(s) + 3/2O2(g) ΔH= 1648.4/2 kJ --------------(5)
reverse (3)
3Fe(s) + 2O2(g) --> Fe3O4(s) ΔH= -1118.4 kJ --------------(6)
Add (4) (5) (6)
FeO(s) --> Fe(s) + 1/2O2(g) ΔH = 272.0 kJ
Fe2O3(s) --> 2Fe(s) + 3/2O2(g) ΔH= 824.2 kJ
3Fe(s) + 2O2(g) --> Fe3O4(s) ΔH= -1118.4 kJ
Now
FeO(s) + Fe2O3(s) --> Fe3O4(s)
ΔH= 272.0 kJ + 824.2 kJ -1118.4 kJ
= -22.2 kJ
Question 10 Calculate AHpxn for the reaction below given: AH+ (AsH3(g) - 66.4 kJ/mol; AH [HAS...
Lizi Saved Calculate the Arxn for the following reaction. (AHf[AsH3(g)] = 66.4 kJ/mol; AHf [H3AsO4(aq)] = -904.6 kJ/mol; AHF [H20[1] = -285.8 kJ/mol H3ASO4(aq) + 4H2(0) -- AsH3(g) + 4H20(1) Multiple Choice -685.2 kJ 685.2 kJ O -1981.4 kJ O
What is AH°rxn for the following reaction? H3AsO4(aq) + 4H2(g) → AsH3(g) + 4H2O(1) Substance AH°f(kJ/mol) 171.5 AsH3(8) H3ASO4(aq) H2O(1) -904.6 -285.8 O -790.3 kJ/mol O-1018.9 kJ/mol 0 -410.1 kJ/mol O -67.1 kJ/mol 0 -1876.3 kJ/mol
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