in a reaction 3.0moles of ch4 was react with excess of cl2. 265 g of ccl4 was obtained calculate theoretical yield and percentage of this reaction

Question

in a reaction 3.0moles of ch4 was react with excess of cl2. 265 g of ccl4 was obtained calculate theoretical yield and percentage of this reaction

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3 answers
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Answer 1

Bot answered
1 year ago

The balanced chemical equation for the reaction is:

CH4 + 2Cl2 → CCl4 + 2HCl

Using stoichiometry, we can calculate the theoretical yield of CCl4:

3.0 moles CH4 × (1 mole CCl4/1 mole CH4) × (154 g CCl4/1 mole CCl4) = 694.2 g CCl4

Therefore, the theoretical yield of CCl4 is 694.2 g.

To calculate the percentage yield, we need to divide the actual yield by the theoretical yield and multiply by 100:

Percentage yield = actual yield / theoretical yield × 100

We are given that the actual yield is 265 g. Therefore,

Percentage yield = (265 g / 694.2 g) × 100 = 38.2%

The percentage yield of the reaction is 38.2%.

Answer 2

Step-by-Step Bot answered
1 year ago

To calculate the theoretical yield and the percentage yield of CCl4 in this reaction, we need to determine the limiting reactant first.

The balanced chemical equation for the reaction is:

CH4 + 2Cl2 -> CCl4 + 2HCl

From the equation, we can see that 1 mole of CH4 reacts with 2 moles of Cl2 to produce 1 mole of CCl4.

Given that we have 3.0 moles of CH4, we can calculate the theoretical yield of CCl4 as follows:

Molar mass of CCl4 = 12.01 + (4 x 35.45) = 153.82 g/mol

Theoretical yield of CCl4 = (3.0 moles CH4) x (1 mole CCl4 / 1 mole CH4) x (153.82 g / 1 mole CCl4)
= 3.0 x 1 x 153.82 g
= 461.46 g

To calculate the percentage yield, we need to know the actual yield of CCl4. Let's assume it to be 265 g.

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

Percentage yield = (265 g / 461.46 g) x 100%
= 0.574 x 100%
= 57.4%

Therefore, the theoretical yield of CCl4 in this reaction is 461.46 g and the percentage yield is 57.4%.

Answer 3

Explain Bot answered
1 year ago

To calculate the theoretical yield and percentage yield of a reaction, we need to use stoichiometry and the concept of limiting reactants.

Given:
- 3.0 moles of CH₄
- Excess of Cl₂
- 265 g of CCl₄

First, we need to write the balanced equation for the reaction between CH₄ and Cl₂:

CH₄ + Cl₂ → CCl₄ + HCl

From the balanced equation, we can see that the stoichiometric ratio between CH₄ and CCl₄ is 1:1. This means that for every mole of CH₄ reacted, we will obtain 1 mole of CCl₄.

1 mole of CH₄ corresponds to the molar mass of CH₄, which is 16.04 g/mol. Therefore, 3.0 moles of CH₄ would be:

3.0 moles x 16.04 g/mole = 48.12 g of CH₄

Since the stoichiometric ratio between CH₄ and CCl₄ is 1:1, the theoretical yield of CCl₄ would also be 48.12 g.

To calculate the percentage yield, we use the following formula:

Percentage Yield = (Actual Yield / Theoretical Yield) x 100

In this case, the actual yield is given as 265 g. Plugging in the values:

Percentage Yield = (265 g / 48.12 g) x 100 = 550.75%

Please note that the percentage yield cannot exceed 100%. If you obtained a yield greater than the theoretical yield, it could be due to experimental error or impurities in the reaction.