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22/09/2021
The theoretical yield is 91.5g of ##NaCl##
Method 1
Start with the equation:
##2Na_((s))+Cl_(2(g))rarr2NaCl_((s))##
So 2 mole ##Na## reacts with 1 mole ##Cl_2## to give 2 moles##NaCl##
Convert moles to grams: ##A_r Na=23## ##A_rCl=35.5##
2×23 = 46g ##Na## reacts with 2x 35.5 = 71g ## Cl_2## to give 2x(23 +35.5 ) = 117g ##NaCl##
Use simple proportion to find how much would be made from 36g ##Na## by first working out what 1 g of ##Na## would give by dividing through by 46:
(46/46)g ##Na## reacts with (71/46) g ##Cl_2## to give (117/46)g ##NaCl##
So:
1g ##Na## reacts with 1.54g ##Cl_2## to give 2.54g ##NaCl##
So:
36g ##Na## reacts with 1.54×36= 55.44g ##Cl_2## to give 2.54×36=91.44g ##NaCl##
You can see that the chlorine is in excess so the theoretical yield is 91.5g of ##NaCl## to 1sf.
Method 2
Start with the balanced equation as above. Calculate the amount of NaCl that can form from each reactant.
36.0 g Na × ##”1 mol Na”https://studydaddy.com/”22.99 g Na” × “2 mol NaCl”https://studydaddy.com/”2 mol Na”## = 1.566 mol NaCl (3 significant figures + 1 guard digit)
75.2 g Cl₂ × ##(“1 mol Cl”_2)/(“70.91 g Cl”_2) × “2 mol NaCl”/(“1 mol Cl”_2)## = 2.121 mol NaCl
The Na gives fewer moles of NaCl, so Na is the limiting reactant.
The theoretical yield is
1.566 mol NaCl × ##”58.44 g NaCl”https://studydaddy.com/”1 mol NaCl” =” 91.5 g NaCl”##
Method 3
Divide the moles of each reactant by its coefficient in the balanced equation.
36.0 g Na × ##”1 mol Na”https://studydaddy.com/”22.99 g Na” =” 1.566 mol Na”## (3 significant figures + 1 guard digit)
75.2 g Cl₂ × ##(“1 mol Cl”_2)/(“70.91 g Cl”_2) =” 2.121 mol Cl”_2##
##2″Na” + “Cl”_2 → 2″NaCl”##
##1.566/2##; ##2.121/1##
0.7829; 2.121
NaCl gives fewer “moles of reaction”, so NaCl is the limiting reactant.
So theoretical yield is
0.7829 mol reaction × ##”2 mol NaCl”https://studydaddy.com/”1 mol reaction” × “58.44 g NaCl”https://studydaddy.com/”1 mol NaCl”## = 91.5 g NaCl
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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