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Rom the following balanced equation, 2al(s) 3cl2(g)⟶2alcl3(s) how many moles of cl2 are required to form 3.55mol alcl3? A. 5.33 mol

B. 2.67 mol
C. 3.55 mol
D. 7.10 mol

User Artanis
by
8.2k points

1 Answer

3 votes

The answer is A. 5.33 mol.

How to find moles?

To determine the number of moles of Cl₂ required to form 3.55 mol of AlCl₃, use the stoichiometric coefficients from the balanced chemical equation:

2Al(s) + 3Cl₂(g) ⟶ 2AlCl₃(s)

This equation tells us that 3 moles of Cl₂ are required to react with 2 moles of AlCl₃. Therefore, set up a proportion:

3 moles Cl₂ / 2 moles AlCl₃ = x moles Cl₂ / 3.55 moles AlCl₃

Solving for x:

x = (3 moles Cl₂/2 moles AlCl₃) × (3.55 moles AlCl₃)

x = 5.33 moles Cl₂

Therefore, 5.33 moles of Cl₂ are required to form 3.55 mol of AlCl₃.

Complete question:

Using the following balanced equation, 2al(s) 3cl2(g)⟶2alcl3(s) how many moles of cl2 are required to form 3.55mol alcl3?

A. 5.33 mol

B. 2.67 mol

C. 3.55 mol

D. 7.10 mol

User Tom Honermann
by
7.9k points
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