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Calculate the approximate enthalpy change, ΔHrxn, for the combustion of methane: CH4+2O2→2H2O+CO2 ΔHrxn from a given table: CH4 = 1656 kJ/mol O2 = 498 kJ/mol H2O = 928 kJ/mol CO2 = 1598 kJ/mol ΔHrxn = [(1656) + (2*498)] - [(2*928) + (1598)] = -802 kJ/mol ?

Zach Chandler

in Chemistry

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Karen Wright on January 15, 2019

We subtract the enthalpies of the products on the part of the enthalpies of the reactants, taking into account their stoichiometric coefficients:2ΔH(H2O) + ∆ H(CO2) - ∆ H(CH4) - ∆ H(2O2)= 2(928) + 1598 - 1656 - 2(498)= 802 kJ / 1 mol of methane


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