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Question: For the balanced equation 4C6H5Cl + 29O2 --> 24CO2 + 10H2O + 2Cl2, if the reaction of 39.3 grams of C6H5Cl produced 11.3 grams of H2O, what is the percent yield?
Step One: Identify the limiting reagent. (the question only gives you one of the reactants, therefore, making that compound the limiting reagent)
The limiting reagent is C6H5Cl.
Step Two: Find the theoretical yield.
Question: For the balanced equation 4C6H5Cl + 29O2 --> 24CO2 + 10H2O + 2Cl2, if the reaction of 39.3 grams of C6H5Cl produced 11.3 grams of H2O, what is the percent yield?
Step One: Identify the limiting reagent. (the question only gives you one of the reactants, therefore, making that compound the limiting reagent)
The limiting reagent is C6H5Cl.
Step Two: Find the theoretical yield.
Here are the steps to finding the theoretical yield
Step One: Use the limiting reagent and see what the ratio is between that and the compound in the product (this is what you are trying to figure out). Make this ratio 1:? or ?:1
Since the limiting reagent is C6H5Cl and the balanced equation is 4C6H5Cl + 29O2 --> 24CO2 + 10H2O + 2Cl2, the ratio between C6H5Cl and H2O is a 4:10 or a 1:2.5 ratio.
Step Two: Using the ratio between the limiting reagent and the compound in the product, find the number of moles in the product's compound by multiplying/diving the limiting reagent by the non-one number in the ratio (1:?).
For every 0.349 moles of C6H5Cl (^number of moles of C6H5Cl that we have^) we need 2.5 times as many moles of H2O, as shown in the ratio, therefore, we multiply the number of moles of C6H5Cl by 2.5 to get 0.873 moles of H2O.
Step Three: Once you know how many moles of the compound in the product you have, turn the moles back into grams. This allows you to answer the question of how much of ___ compound is able to be produced.
To turn the moles back into grams we used the equation grams=(moles)(GFW).
GFW of H2O: H: (2x1) + O: (1x16) = 18 GFW grams=(0.873moles)(18GFW) ---> grams=15.714g
Step One: Use the limiting reagent and see what the ratio is between that and the compound in the product (this is what you are trying to figure out). Make this ratio 1:? or ?:1
Since the limiting reagent is C6H5Cl and the balanced equation is 4C6H5Cl + 29O2 --> 24CO2 + 10H2O + 2Cl2, the ratio between C6H5Cl and H2O is a 4:10 or a 1:2.5 ratio.
Step Two: Using the ratio between the limiting reagent and the compound in the product, find the number of moles in the product's compound by multiplying/diving the limiting reagent by the non-one number in the ratio (1:?).
For every 0.349 moles of C6H5Cl (^number of moles of C6H5Cl that we have^) we need 2.5 times as many moles of H2O, as shown in the ratio, therefore, we multiply the number of moles of C6H5Cl by 2.5 to get 0.873 moles of H2O.
Step Three: Once you know how many moles of the compound in the product you have, turn the moles back into grams. This allows you to answer the question of how much of ___ compound is able to be produced.
To turn the moles back into grams we used the equation grams=(moles)(GFW).
GFW of H2O: H: (2x1) + O: (1x16) = 18 GFW grams=(0.873moles)(18GFW) ---> grams=15.714g
Step Three: Plug in known information into equation shown below
Percentage Yield = (Actual Yield/Theoretical Yield) x 100%
Percentage Yield = (11.3grams/15.714) x 100%
Percentage Yield = 71.9%
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Percentage Yield = (Actual Yield/Theoretical Yield) x 100%
Percentage Yield = (11.3grams/15.714) x 100%
Percentage Yield = 71.9%
click here to go back to the quiz