Question

Example 3 Calculate the heat released when 5.00 g of aluminum reacts with a stoichiometric amount of iron(III) oxide. 2Al(s) + Fe$_2$O$_3$(g) $\longrightarrow$ 2 Fe(s) + Al$_2$O$_3$(s) $\Delta H^\circ = -852$ kJ

          Example 3
Calculate the heat released when 5.00 g of aluminum reacts with a
stoichiometric amount of iron(III) oxide.
2Al(s) + Fe$_2$O$_3$(g) \(\longrightarrow\) 2 Fe(s) + Al$_2$O$_3$(s) 
$\Delta H^\circ = -852$ kJ

Example 3
Calculate the heat released when 5.00 g of aluminum reacts with a
stoichiometric amount of iron(III) oxide.
2Al(s) + Fe2O3(g) ⟶ 2 Fe(s) + Al2O3(s)
Δ H^∘ = -852 kJ

Added by Denise S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sima Sarker

02/16/2022

Step 1

00 g Molar mass of aluminum (Al) = 26.98 g/mol Number of moles of aluminum = mass / molar mass Number of moles of aluminum = 5.00 g / 26.98 g/mol Number of moles of aluminum = 0.185 moles Show more…

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Example 3 Calculate the heat released when 5.00 g of aluminum reacts with a stoichiometric amount of iron(III) oxide. 2Al(s) + Fe2O3(s) -> 2Fe(s) + Al2O3(s) H = -852 kJ