How many moles of SbCl₃ is formed when 4.00 mol Sb are reacted with 4.43 mol Cl₂ according to the unbalanced equation

Question

Quizplus · Accepted Answer

The balanced equation for the reaction between Sb and Cl2 is:
2Sb + 3Cl2 → 2SbCl3
From the equation, we can see that 2 moles of Sb react with 3 moles of Cl2 to produce 2 moles of SbCl3.
Using mole-to-mole ratio, we can calculate the moles of SbCl3 that will be produced when 4.00 moles of Sb reacts with 4.43 moles of Cl2:
4.00 mol Sb × (2 mol SbCl3/2 mol Sb) = 4.00 mol SbCl3
We can also calculate the moles of SbCl3 that will be produced from the given amount of Cl2:
4.43 mol Cl2 × (2 mol SbCl3/3 mol Cl2) = 2.95 mol SbCl3
The limiting reactant in this reaction is Cl2, since it produces less moles of SbCl3. Therefore, the number of moles of SbCl3 that will be formed is 2.95 mol. Thus, the answer is C.

How Many Moles of SbCl3 Is Formed When 4

How Many Moles of SbCl₃ Is Formed When 4