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
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%.
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%.
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.