Math  /  Algebra

Question\text{How much heat is produced when 74 grams of Al react in the following reaction?} \\ 2 \mathrm{Al}(s) + \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \rightarrow 2 \mathrm{Fe}(s) + \mathrm{Al}_{2} \mathrm{O}_{3}(s) \\ \text{Heat of reaction} = -851.5 \, \mathrm{kJ} \\

Studdy Solution
Use stoichiometry to find the heat produced.
According to the balanced equation, 2 moles of Al\text{Al} produce 851.5kJ-851.5 \, \text{kJ} of heat.
Calculate the heat produced for 2.74 moles of Al\text{Al}: Heat produced=(851.5kJ2mol)×2.74mol\text{Heat produced} = \left(\frac{-851.5 \, \text{kJ}}{2 \, \text{mol}}\right) \times 2.74 \, \text{mol} Heat produced1166.5kJ\text{Heat produced} \approx -1166.5 \, \text{kJ}
The heat produced when 74 grams of aluminum react is approximately 1166.5kJ-1166.5 \, \text{kJ}.

View Full Solution - Free
Was this helpful?

Studdy solves anything!

banner

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

ParentsInfluencer programContactPolicyTerms
TwitterInstagramFacebookTikTokDiscord