SbCl3SbCl3 is a reagent for detecting vitamin A.How many moles of SbCl3SbCl3 are formed when 4.164.16 mol SbSb is reacted with 5.04 mol Cl2Cl2 according to the equation2Sb(s)+3Cl2(g)→2SbCl3(s)
Question
SbCl3SbCl3 is a reagent for detecting vitamin A.How many moles of SbCl3SbCl3 are formed when 4.164.16 mol SbSb is reacted with 5.04 mol Cl2Cl2 according to the equation2Sb(s)+3Cl2(g)→2SbCl3(s)
Solution
The balanced chemical equation is:
2Sb(s) + 3Cl2(g) → 2SbCl3(s)
From the balanced equation, we can see that 2 moles of Sb react with 3 moles of Cl2 to form 2 moles of SbCl3.
Given that we have 4.16 moles of Sb and 5.04 moles of Cl2, we first need to determine which is the limiting reactant, as this will determine how much SbCl3 can be formed.
The mole ratio of Sb to Cl2 is 2:3. So for every 2 moles of Sb, we need 3 moles of Cl2.
If we have 4.16 moles of Sb, we would need 4.16 * (3/2) = 6.24 moles of Cl2 to react completely. But we only have 5.04 moles of Cl2.
Therefore, Cl2 is the limiting reactant.
The mole ratio of Cl2 to SbCl3 is 3:2. So for every 3 moles of Cl2, we can form 2 moles of SbCl3.
So if we have 5.04 moles of Cl2, we can form 5.04 * (2/3) = 3.36 moles of SbCl3.
Therefore, 3.36 moles of SbCl3 are formed when 4.16 mol Sb is reacted with 5.04 mol Cl2.
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