The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product.
Consider the reaction:
CH4(g) + CCl4(g) → 2
CH2Cl2(g)
If 17.38 g CH4 is mixed with 13.50 g CCl4, calculate the theoretical yield (g) of CH2Cl2 produced by the reaction.
Molar mass of CH4,
MM = 1*MM(C) + 4*MM(H)
= 1*12.01 + 4*1.008
= 16.042 g/mol
mass(CH4)= 17.38 g
use:
number of mol of CH4,
n = mass of CH4/molar mass of CH4
=(17.38 g)/(16.04 g/mol)
= 1.083 mol
Molar mass of CCl4,
MM = 1*MM(C) + 4*MM(Cl)
= 1*12.01 + 4*35.45
= 153.81 g/mol
mass(CCl4)= 13.5 g
use:
number of mol of CCl4,
n = mass of CCl4/molar mass of CCl4
=(13.5 g)/(1.538*10^2 g/mol)
= 8.777*10^-2 mol
Balanced chemical equation is:
CH4 + CCl4 ---> 2 CH2Cl2
1 mol of CH4 reacts with 1 mol of CCl4
for 1.083 mol of CH4, 1.083 mol of CCl4 is required
But we have 8.777*10^-2 mol of CCl4
so, CCl4 is limiting reagent
we will use CCl4 in further calculation
Molar mass of CH2Cl2,
MM = 1*MM(C) + 2*MM(H) + 2*MM(Cl)
= 1*12.01 + 2*1.008 + 2*35.45
= 84.926 g/mol
According to balanced equation
mol of CH2Cl2 formed = (2/1)* moles of CCl4
= (2/1)*8.777*10^-2
= 0.1755 mol
use:
mass of CH2Cl2 = number of mol * molar mass
= 0.1755*84.93
= 14.91 g
Answer: 14.91 g
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