A visual representation of a chemical reaction. On the left side, depict 2 molecules of methane (CH4), represented as tetrahedral molecules with a central carbon atom connected to four hydrogen atoms. Surround these molecules with an excess of chlorine gas (Cl2) molecules, each represented as two green balls connected by a line. On the right side of the image, depict an arrow leading to a complex molecule represented as carbon tetrachloride (CCl4). This molecule should be shown as one large carbon atom at the center connected to four smaller chlorine atoms. Make sure no text is included in the illustration.

In a reaction 2 moles of CH4 were reacted with an excess of Cl2. As a result 117gram of CCl4 is obtained. What is theoratical yield?

Actual yield?
%age yield?

CH4 + 4Cl2 → CCl4 + 4HCl

2 mols CH4 will produce 2 mols CCl4.
2 mols CCl4 has a mass of 2*[12 + 4*35.5] = 308 g.That is the theoretical yield.
actual yield = 117 grams = AY
theoretical yield = 308 grams = TY
%yield = (AY/TY)*100 = ?

@oobleck. 2 mol CCl4 = 2*154 = 308 g

We should outlaw all coefficients.

2CH4 + 4Cl2 = 2CCl4 + 4H2

the theoretical yield is 2 moles of CCl4, or 154g
You got 117g, or 117/154 = 76%

dang those pesky coefficients!

Well, well, well! Looks like you've got a reaction on your hands, and not the emotional kind. Let's dive right into it with some clown chemistry!

Now, according to the reaction, we have 2 moles of CH4 and excess Cl2. To figure out the theoretical yield, we need to know the molar mass of CCl4, which is approximately 153.8 g/mol.

First, let's calculate the theoretical yield:

2 moles of CH4 x (1 mole of CCl4 / 1 mole of CH4) x (153.8 g of CCl4 / 1 mole of CCl4) = X grams of CCl4

Now, since this is theoretical, we're assuming everything goes perfectly, like a circus performer nailing every trick. But in reality, we know that life isn't always a three-ring circus, and sometimes things don't go as planned. So, let's move on and see what really happened!

Given that 117 grams of CCl4 were obtained, that's our actual yield. No grand illusions or trickery here!

Now, let's calculate the percentage yield using the formula:

% yield = (Actual Yield / Theoretical Yield) x 100

Plug in the values:

% yield = (117 g / X g) x 100

Now, it's time for you to plug in the value of X (the theoretical yield) and calculate the final result. Remember, the actual yield could be less, but don't let that bring you down. The percentage yield will reveal just how close to perfect your reaction was!

I hope my clowning around with chemistry helped make this topic a little more amusing for you. Happy calculating!

To determine the theoretical yield, we need to calculate the amount of CCl4 that can be produced assuming the reaction goes to completion.

First, we need to find the molar mass of CH4 (methane) and CCl4 (carbon tetrachloride):

Molar mass of CH4 = 12.01 g/mol (molar mass of carbon) + 4 * 1.01 g/mol (molar mass of hydrogen) ≈ 16.05 g/mol
Molar mass of CCl4 = 12.01 g/mol (molar mass of carbon) + 4 * 35.45 g/mol (molar mass of chlorine) ≈ 153.82 g/mol

We know that 1 mole of CH4 reacts with 1 mole of Cl2 to produce 1 mole of CCl4. Therefore, 2 moles of CH4 will produce 2 moles of CCl4.

Now, let's calculate the theoretical yield:

Theoretical yield (in grams) = moles of CCl4 * molar mass of CCl4
Theoretical yield = 2 moles * 153.82 g/mol ≈ 307.64 g

To calculate the actual yield, you need the information provided in the question. It states that 117 grams of CCl4 is obtained. Therefore, the actual yield is 117 grams.

To calculate the percentage yield, use the formula:

% yield = (actual yield / theoretical yield) * 100

% yield = (117 g / 307.64 g) * 100 ≈ 38.05%

Therefore, the theoretical yield is approximately 307.64 grams, the actual yield is 117 grams, and the percentage yield is approximately 38.05%.