Determine the limiting reaction, number of moles of the excess reactant?

Consider the reaction:





2Sb(s) + 3Cl2 (g) -----%26gt; 2SbCl3 (s)





Determine the limiting reaction and the number of moles of the excess reactant remaining when 2 moles of antimony and 2 moles of chlorine gas react.





A.) antimony and 2 moles of chlorine remain


B.) antimony and 4 moles of chlorine remain


C.) chlorine and 3 moles of antimony remain


D.) chlorine and 4 moles of antimony remain


E.) chlorine and 2 moles of antimony remain








please show how you go it!

Determine the limiting reaction, number of moles of the excess reactant?
via stoichiometric ratio 2 mols of Sb requires 3 mols of Cl for complete reaction. there is clearly not enough Cl so that is the limiting reagent.





by the same ratio, 2mols of Cl requires 1.33 mols of Sb. the excess reagent is 0.667mol of Sb. this is the correct answer.





F) None of the above.
Reply:for the reaction the molar ratio of product to reactant is:





(1 mole of SbCL3/1 mole Sb) and


(2 mole of SbCL3/3 mole Cl2)





We have 2 moles of Sb, therefore at most could make:





(2 mole Sb)* (1 mole SbCL3/1 mole Sb) = 2 mole SbCL3





We have 2 moles of CL2, therefore at most could make:





(2 moles CL2)* (2 mole SbCl3/3 mole CL2) = 4/3 mole SbCL3





The limiting reactant is the chlorine


(4/3 mole SbCl3)*(1 mole Sb/1 mole SbCL3) = 4/3 mole Sb used, therefore 2/3 mole of Sb remains
Reply:taking the equation on a surface lvl.....


the mole ration in the equation is 2:3 of Sb to Cl.





thus, if u say2 mole of Sb and 2 mole of Cl, then the new mole ration becomes?....4:6 of Sb to Cl. from the ration now it obvius that while there is lot of Cl to react, there is not enough Sb. so 4 of Sb will react with 4 of Cl.





meaning that the Sb is the limiting reactant





and 6-4= 2 OF Cl , meaning that 2 moles of excess Cl





the correct answere is (A)

night jasmine