Question

In: Chemistry

For the reaction shown, compute the theoretical yield of the product in grams for each of...

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

Solutions

Expert Solution

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


Related Solutions

For the reaction shown, compute the theoretical yield of product (in grams) for each of the...
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) A) 2.5 g Al, 2.5 g Cl2 B) 7.7 g Al, 24.6 g Cl2 C) 0.235 g Al, 1.20 g Cl2
For the reaction shown, compute the theoretical yield of product (in grams) for each of the...
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) A) 2.5 g Al, 2.5 g Cl2 B) 7.7 g Al, 24.6 g Cl2 C) 0.235 g Al, 1.20 g Cl2
For the reaction shown, compute the theoretical yield of the product in grams for each of...
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) 1) 1.0 gAl; 1.0 gCl2 Express your answer using two significant figures. 2) 5.5 gAl; 19.8 gCl2 Express your answer using three significant figures. 3) 0.439 gAl; 2.29 gCl2 Express your answer using three significant figures.
For the reaction shown, compute the theoretical yield of the product in grams for each of...
For the reaction shown, compute the theoretical yield of the product in grams for each of the following initial amounts of reactants. Ti(s)+2F2(g)→TiF4(s) 1.0 gTi; 1.0 gF2 Express your answer using two significant figures. 4.8 gTi; 3.2 gF2 Express your answer using two significant figures. 0.388 gTi; 0.341 gF2 Express your answer using three significant figures.
For the reaction shown, compute the theoretical yield of the product in grams for each of...
For the reaction shown, compute the theoretical yield of the product in grams for each of the following initial amounts of reactants. Ti(s)+2F2(g)→TiF4(s) a. 1.0 gTi; 1.0 gF2 b. 4.8 gTi; 3.2 gF2 c. 0.388 gTi; 0.341 gF2 Express your answer using two significant figures.
For the reaction shown, compute the theoretical yield of product (in grams) for each of the...
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) Part B 7.8 g Al, 25.2 g Cl2 Express your answer using three significant figures. Part C 0.230 g Al, 1.10 g Cl2 Express your answer using three significant figures.
For the reaction shown, compute the theoretical yield of the product (in grams) for each of...
For the reaction shown, compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants. Ti(s)+2F2(g)→TiF4(s) 1)7.0 g Ti , 7.0 g F2 Express your answer using two significant figures. m= ______ g 2) 2.3 g Ti , 1.5 g F2 Express your answer using two significant figures. m=_______ g 3) 0.236 g Ti , 0.292 g F2 M =_____ g   
For the reaction shown, compute the theoretical yield of product (in grams) for each of the...
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) 1) 7.7 g Al, 24.4 g Cl2 Express your answer using three significant figures. 2)0.230 g Al, 1.15 g Cl2 Express your answer using three significant figures.
For the reaction shown, compute the theoretical yield of the product in moles for each of...
For the reaction shown, compute the theoretical yield of the product in moles for each of the initial quanities of reactants. Ti(s)+ 2Cl2(g)=TiCl4(s) A) 2 mol Ti, 2 mol Cl2 express your answer using two significant figures. B) 5 mol Ti, 9 mol Cl2 express your answer using two significant figures. C) 0.483 mol Ti, 0.911 mol Cl2 express your answer using three significant figures. D) 12.4 mol Ti, 15.8 mol Cl2 express your answer using three significant figures
For the reaction Ti(s)+2F2(g)→TiF4(s) compute the theoretical yield of the product (in grams) for each of...
For the reaction Ti(s)+2F2(g)→TiF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants. Part A 4.0 g Ti, 4.0 g F2 Part B 2.3 g Ti, 1.4 g F2 Part C 0.227 g Ti, 0.293 g F2
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT