Question

When 15.0 g of chlorine is added to acetylene, C2H2, 16.8 g of 1,1,2,2-tetrachloroethane, C2H2Cl4, is formed:

2 Cl2 (g) + C2H2 (g) → C2H2Cl4 (l)


What is the percent yield of this reaction?

Answer 1

94.6%

Step-by-step explanation:

Step 1:

The balanced equation for the reaction. This is given below:

2Cl2(g) + C2H2(g) → C2H2Cl4(l)

Step 2:

Determination of the mass of Cl2 that reacted and the mass of C2H2Cl4 produced from the balanced equation.

This is illustrated below:

Molar Mass of Cl2 = 2 x 35.5 = 71g/mol

Mass of Cl2 from the balanced equation = 2 x 71 = 142g

Molar Mass of C2H2Cl4 = (12x2) + (2x1) + (35.5x4) = 168g.

Mass of C2H2Cl4 from the balanced equation = 1 x 168 = 168g

Therefore, 146g of Cl2 reacted and 168g of C2H2Cl4 were produced from the balanced equation.

Step 3:

Determination of the theoretical yield of C2H2Cl4.

This is illustrated below:

From the balanced equation above,

146g of Cl2 reacted to produce 168g of C2H2Cl4.

Therefore, 15g of Cl2 will react to produce = (15 x 168)/142 = 17.75g of C2H2Cl4.

Therefore, the theoretical yield of C2H2Cl4 is 17.75g

Step 4:

Determination of the percentage yield of C2H2Cl4.

The percentage yield of C2H2Cl4 can be obtained as follow:

Actual yield of C2H2Cl4 = 16.8g

Theoretical yield of C2H2Cl4 = 17.75g

Percentage yield of C2H2Cl4 =..?

Percentage yield = Actual yield /Theoretical yield x 100

Percentage yield = 16.8/17.75 x 100

Percentage yield = 94.6%

Therefore, the percentage yield of C2H2Cl4 is 94.6%

Answer 2

`Y=84.5\%`

Step-by-step explanation:

Hello,

In this case, given the reaction, we can compute the moles of chlorine that are consumed and the yielded grams of 1,1,2,2-tetrachloroethane by using their molar masses, 70.9 g/mol and 167.8 g/mol respectively by using their 2:1 molar ratio:

`m_(C_2H_2Cl_4 )=15.0gCl_2*(1molCl_2)/(70.9gCl_2)*(1molC_2H_2Cl_4 )/(2molCl_2) *(167.8gC_2H_2Cl_4 )/(1molC_2H_2Cl_4 ) \\\\m_(C_2H_2Cl_4 )=17.75gC_2H_2Cl_4`

Then we compute the percent yield:

`Y=(15.0g)/(17.75g)*100\%\\ \\Y=84.5\%`

Best regards.