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[" a series of complex bio-chemical reac...

[" a series of complex bio-chemical reactions "],[" involving enzymes."],[" Problem 6.9"],[" The combustion of one mole of benzene "],[" takes place at "298K" and "1" atm.After "],[" combustion,"CO_(2)(g)" and "H_(2)O" (1) are "],[" produced and "3267.0kJ" of heat is "],[" liberated.Calculate the standard "],[" enthalpy of formation,"Delta_(f)H^(ominus)" of benzene."],[" Standard enthalpies of formation of "],[CO_(2)(g)" and "H_(2)O(1)" are "-393.5kJmol^(-1)],[" and "-285.83kJmol^(-1)" respectively."]

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The combustion of 1 mole of benzene takes place at 298K and 1 atm. After combustion, CO_(2(g)) and H_(2)O_((l)) are produced and 3267.0 KJ of heat is liberated. Calculate the standard enthalpy of formation, Delta_(f)H^(0) of benene. Standard enthalpies of formation of CO_(2(g))andH_(2)O_((l)) are -393.5 KJ mol^(-1) and - 285.83 KJ mol^(-1) respectively

The combustion of one mole of benzene takes place at 298 and 1 atm. After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation. triangle_f H^@ benzene. Standard enthalpies of formation of CO_2(g) and H_20(l) are -393,5 kJ mol ""^(-1) and "-285.83 kJ mol"^(-1) respectively.

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

Calculate the standard enthalpy of formation of propane (C_(3)H_(8)) if its enthalpy of combustion is -2220.2 kJ "mol"^(-1) .The enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5 and -285.8 kJ "mol"^(-1) respectively.

The combustion of butane (C_(4)H_(10)) is exothermic by 2878.7 kJ "mol"^(-1) .Calculate the standard enthalpy of formation of butane given that the standard enthalpies of formation of CO_(2)(g) and H_(2)O(l) are -393.5 kJ "mol"^(-1) and -285.8 kJ "mol"^(-1) respectively.

Calculate the standard enthalpy of formation of n- butane. Given : standard enthalpy of combustion of n- butane, C (graphite) and H_(2)(g) " are " -2878.5 " kJ mol"^(-1), -393.5 " kJ mol"^(-1) and -285.8 " kJ mol"^(-1) respectively.

Calculate the standard enthalpy of combustion of CH_(4) , it standard enthalpies of formation of CH_(4(g)),H_(2)O_((l)), and CO_(2(g)) are -74.81kJ mol^(-1), -285.83kJ mol^(-1) and -393.51kJ mol^(-1) respectively.