In: Chemistry
For the reaction shown, compute the theoretical yield of the product in grams for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s)
A) 1.0 g Al; 1.0 g Cl2
B) 5.5 g Al; 19.8 g Cl2
C) 0.439 g Al; 2.29 g Cl2
As the reaction is given by
2 Al(s) + 3 Cl2(g) --> 2 AlCl3 (s)
molar mass of Al = 27g/mol , molar mass of Cl = 35.5 g/mol , we get
molar mass of Cl2 = 71 g/mol
Now we calculate the no of moles of the reactants
no of moles = given mass / molar mass
1) no of moles of Al = 1 g /27 g/mol = 0.037 moles
no of moles of Cl2 = 1 g /71/mol = 0.014 moles
As , 3 moles of Cl2 react with 2 moles Al to produce 2 moles AlCl3
1 moles of CL2 reacts with 2/3 moles of Al
0.014 moles of CL2 reacts with 0.014 * 0.0246 = 0.0093 moles of Al
CL2 is limiting agent here and some of the AL remains unreacted .
hence yield of the product is
= no of moles * molar mass = 133.5 g /mol * 0.0093 mol = 1.241 g of AlCL3 is formed
2) no of moles of Al = 5.5g / 27 g/mol = 0.203 moles
no of moles of Cl2 = 19.8g / 71g/mol = 0.278 moles
As , 3 moles of Cl2 react with 2 moles Al to produce 2 moles AlCl3
1 moles of CL2 reacts with 2/3 moles of Al
0.203 moles of CL2 reacts with 0.203 * 2/3 = 0.136 moles of Al
CL2 is limiting agent here and some of the AL remains unreacted .
hence yield of the product is
= no of moles * molar mass = 133.5 g /mol * 0.136 mol = 18.156 g ALCL3 is formed
3)
no of moles of Al = 0.439 g / 27 g/mol = 0.0162 moles
no of moles of Cl2 = 2.29 g / 71g/mol = 0.0322 moles
As , 2 moles of Al react with 3 moles CL2 to produce 2 moles AlCl3
1 moles of Al reacts with 2/3 moles of CL2
0.0162 moles of AL reacts with 2/3 * 0.0162 moles of CL2 = 0.0108 moles of CL2
AL is limiting agent here and some of the CL2 remains unreacted .
hence yield of the product is
= no of moles * molar mass = 133.5 g /mol * 0.0162 mol = 2.162 g of ALCL3 is formed