(Solved): The overall reaction in a commercial heat pack can be represented as \[ 4 \mathrm{Fe}(s)+3 \mathrm{ ...

The overall reaction in a commercial heat pack can be represented as \[ 4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \quad \Delta H=-1652 \mathrm{~kJ} \] a. How much heat is released when \( 4.80 \) moles of iron are reacted with excess \( \mathrm{O}_{2} \) ? \[ \text { Heat }=\quad \mathrm{kJ} \] b. How much heat is released when \( 1.00 \) mole of \( \mathrm{Fe}_{2} \mathrm{O}_{3} \) is produced? \[ \text { Heat }=\quad \mathrm{kJ} \] c. How much heat is released when \( 1.70 \mathrm{~g} \) iron is reacted with excess \( \mathrm{O}_{2} \) ? \[ \text { Heat }=\quad \mathrm{kJ} \] d. How much heat is released when \( 12.8 \mathrm{~g} \mathrm{Fe} \) and \( 1.70 \mathrm{~g} \mathrm{O}_{2} \) are reacted? Heat = kJ