Chemistry, 25.02.2020 03:23, tdyson3p6xvtu
Calculate the standard heat of reaction for the following methane-generating reaction of methanogenic bacteria: 4CH3NH2(g) + 2H2O(l) → 3CH4(g) + CO2(g) + 4NH3(g) Given that ΔHfo(CH3NH2, g) = –22.97 kJ/mol; ΔHfo(H2O, l) = –285.8 kJ/mol; ΔHfo(CH4, g) = –74.8 kJ/mol; ΔHfo(CO2, g) = –393.5 kJ/mol ΔHfo(NH3, g) = –46.1 kJ/mol
Answers: 2
![\Delta H^o_{rxn}=\sum [n\times \Delta H_f_{(product)}]-\sum [n\times \Delta H_f_{(reactant)}]](/tpl/images/0522/6322/e893d.png)
![\Delta H_{rxn}=[(3\times \Delta H_f_{(CH_4(g))})+(1\times \Delta H_f_{(CO_2(g))})+(4\times \Delta H_f_{(NH_3(g))})]-[(4\times \Delta H_f_{(CH_3NH_2(g))})+(2\times \Delta H_f_{(H_2O(l))})]](/tpl/images/0522/6322/6730f.png)
![\Delta H_{rxn}=[(3\times (-74.8))+(1\times (-393.5))+(4\times (-46.1))]-[(4\times (-22.97))+(2\times (-285.8))]\\\\\Delta H_{rxn}=-138.82kJ](/tpl/images/0522/6322/fdc01.png)
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