I'm sorry but the answer that you got was incorrect.
Let's go through the steps together to help you understand.
Question: For the balanced equation CBr4 + O2 --> CO2 + 2Br2, if the reaction of 97.4 grams of CBr4 produces a 37.8% yield, how many grams of Br2 would be produced?
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 CBr4
Step Two: Find the theoretical yield.
Question: For the balanced equation CBr4 + O2 --> CO2 + 2Br2, if the reaction of 97.4 grams of CBr4 produces a 37.8% yield, how many grams of Br2 would be produced?
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 CBr4
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 CBr4 and the balanced equation is CBr4 + O2 --> CO2 + 2Br2, the ratio between CBr4 and Br2 is a 1:2 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 0.293 moles of CBr4 (^number of moles of CBr4 that we have^) we need twice as many moles of Br2, as shown in the ratio, therefore, we multiply the number of moles of CBr4 by 2 to get 0.586 moles of Br2.
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 Br2: (2x80) = 160 GFW grams=(0.586moles)(160GFW) ---> grams=93.76g
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 CBr4 and the balanced equation is CBr4 + O2 --> CO2 + 2Br2, the ratio between CBr4 and Br2 is a 1:2 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 0.293 moles of CBr4 (^number of moles of CBr4 that we have^) we need twice as many moles of Br2, as shown in the ratio, therefore, we multiply the number of moles of CBr4 by 2 to get 0.586 moles of Br2.
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 Br2: (2x80) = 160 GFW grams=(0.586moles)(160GFW) ---> grams=93.76g
Step Three: Plug in known information into equation shown below
Percentage Yield = (Actual Yield/Theoretical Yield) x 100%
37.8% = (Actual Yield/93.76grams) x 100%
Actual Yield = 35.441 grams
click here to go back to the quiz
Percentage Yield = (Actual Yield/Theoretical Yield) x 100%
37.8% = (Actual Yield/93.76grams) x 100%
Actual Yield = 35.441 grams
click here to go back to the quiz