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[" Given:: "Fe+3/2O(2)longrightarrow Fe(...

[" Given:: "Fe+3/2O_(2)longrightarrow Fe_(2)O_(3),Delta H=-193.4kJ],[Mg+1/2O_(2)longrightarrow MgO,Delta H=-140.2kJ],[" What is "Delta H" of the reaction- "],[Mg+Fe_(2)O_(3)longrightarrow3MgO+2Fe?],[[" (1) "-227.2kJ," (2) "-272.3kJ],[" (3) "227.2kJ," (4) "272.3kJ]]

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Given: i. 2Fe(s) +(3)/(2)O_(2)(g) rarr Fe_(2)O_(3)(s), DeltaH^(Theta) =- 193.4 kJ ii. Mg(s) +(1)/(2)O_(2)(g) rarr MgO(s), DeltaH^(Theta) =- 140.2kJ What is DeltaH^(Theta) of the reaction? 3Mg +Fe_(2)O_(3)rarr 3MgO +2Fe

Given: i. 2Fe(s) +(3)/(2)O_(2)(g) rarr Fe_(2)O_(3)(s), DeltaH^(Theta) =- 193.4 kJ ii. Mg(s) +(1)/(2)O_(2)(g) rarr MgO(s), DeltaH^(Theta) =- 140.2kJ What is DeltaH^(Theta) of the reaction? 3Mg +Fe_(2)O_(3)rarr 3MgO +2Fe

Delta_(f)H^(@) of Fe_(2)O_(3) is -825 kJ. What is the enthalpy change for the reaction? 4Fe_(2)O_(3) to 8Fe + 6O_(2)

Balance the equation , Fe + H_(2)O to Fe_(3)O_(4) + H_(2)

The heats of oxidation of Mg and Fe are given: Mg+1/2O_2 rarr MgO,Delta H=-145700 cal 2Fe+3/2O_2 rarr Fe_2O_3, Delta H=-193500 cal calculate the heat produced in the reaction 3 Mg+Fe_2O_3=3MgO+2Fe

The heat of formation of Fe_(2)O_(3) is -824.2 kJ mol^(-1). Delta H for the reaction 2Fe_(2)O_(3)(s)rarr 4Fe(s)+3O_(2)(g) is :