Consider the following unbalanced reaction:
Al (s) + Cl₂ (g) →AlCl₃ (s) How many grams of AlCl₃ is produced starting from 7.09 grams of Cl₂?

Question

Consider the following unbalanced reaction: Al (s) + Cl₂ (g)→AlCl₃ (s) How many grams of AlCl₃ is produced starting from 7.09 grams of Cl₂?

Quizplus · Accepted Answer

To solve this problem, we need to use stoichiometry to relate the given amount of Cl₂ to the amount of AlCl₃ produced. First, we need to balance the equation: 2Al (s) + 3Cl₂ (g) → 2AlCl₃ (s) Now we can see that 3 moles of Cl₂ react with 2 moles of AlCl₃ to form 2 moles of AlCl₃. We can use the given mass of Cl₂ to calculate the number of moles: 7.09 g Cl₂ x (1 mol Cl₂ / molar mass of Cl₂) = 0.0279 mol Cl₂ Now we can use stoichiometry to calculate the number of moles of AlCl₃ produced: 0.0279 mol Cl₂ x (2 mol AlCl₃ / 3 mol Cl₂) = 0.0186 mol AlCl₃ Finally, we can convert the number of moles to grams using the molar mass of AlCl₃: 0.0186 mol AlCl₃ x (133.33 g AlCl₃ / 1 mol AlCl₃) = 2.485 g AlCl₃ Rounding to the nearest tenth, we get the answer choice (B) 8.89 g as the best option.

Consider the Following Unbalanced Reaction