Question 10 of 10 Incorrect Map Sapling Learning macmillan l

Question 10 of 10 Incorrect Map Sapling Learning macmillan learning Each step in the process below has a 80.0% yield CH4 +4Cl2 CCl4 + 2 HF CCl4 +4HCI CCLF2 + 2HCl The CCl4 formed in the first step is used as a reactant in the second step If 4.00 mol of CH4 reacts, what is the total amount of HCI produced? Assume that Cl2 and HF are present in excess Number mol HCI Tools x 102 Previous Check Answer @NextExit Hint

Solution

Ans. Step 1: Balanced reaction:      CH₄ + 4Cl₂ ------> CCl₄ + 4 HCl.

According to the stoichiometry of balanced reaction, 1 mol CH₄ produces 1 mol CCl₄ and 4 mol HCl.

So, starting from 4.0 mol CH₄ and following stoichiometry of balanced reaction-

            Theoretical yield of CCl₄ = 1 x Moles of CH₄ = 1 x 4 mol = 4.0 mol

            Theoretical yield of HCl = 4 x Moles of CH₄ = 4 x 4 mol = 16.0 mol

# Given, experimental yield is 80%.

So,

Experimental yield of CCl₄ = 80% of theoretical yield = 80% of 4.0 mol = 3.2 mol

Experimental yield of HCl = 80% of theoretical yield = 80% of 16.0 mol = 12.8 mol

# Step 2: Balanced reaction:           CCl₄ + 2 HF ------> CCl₂F₂ + 2 HCl.

According to the stoichiometry of balanced reaction, 1 mol CCl₄ produces 1 mol HCl.

# from step #1, available moles of CCl₄ is 3.2 mol.

            Theoretical yield of HCl = 2 x Moles of CCl₄ = 2 x 3.2 mol = 6.4 mol

# Given, experimental yield is 80%.

So,

Experimental yield of HCl = 80% of theoretical yield = 80% of 6.4 mol = 5.12 mol

# Step 3: Total experimental/actual yield of HCl =

Actual yield in step 1 + Actual yield in step 2

= 12.8 mol + 5.12 mol

= 17.92 mol