If the percentage yield is results to 100%, thenA. there was no limiting reactantB. the actual yield is equal to the theoretical yieldC. the actual yield is less than the theoretical yieldD. the actual yield is greater than the theoretical yield
1. If the percentage yield is results to 100%, thenA. there was no limiting reactantB. the actual yield is equal to the theoretical yieldC. the actual yield is less than the theoretical yieldD. the actual yield is greater than the theoretical yield
Answer:
D. the actual yield is greater than the theoretical yield
2. What is the resulting actual yield of 100% yield and an 88g theoretical yield?
Answer:
actual yield = 88 g
Explanation:
Solve for the actual yield.
percent yield = (actual yield / theoretical yield) × 100
actual yield = (percent yield / 100)(theoretical yield)
actual yield = (100 / 100)(88 g)
actual yield = 88 g
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3. Activity No.1 Compute the conversion factor of the following: 1. Old yield = 2 New yield= 20 Conversion Factor= ______ 2. Old Yield = 20 New Yield = 100 Conversion Factor= _____ 3. Old Yield = 4 New Yield = 48 Conversion Factor= 4. Old Yield = 3 New Yield = 15 Conversion Factor= _____ 5. Old Yield = 10 New Yield = 70 Conversion Factor= _____
Answer:
1.-25
2.45
3-32
4-15
5.45
thanks me later
4. If the percent yield of a reaction was 65.0% and its theoretical yield was 0.652 g of CO2 what was the actual yield?
To find the actual yield, we can use the percent yield formula:
percent yield = (actual yield / theoretical yield) x 100%
Rearranging the formula, we can solve for the actual yield:
actual yield = (percent yield / 100%) x theoretical yield
Substituting the given values, we get:
actual yield = (65.0 / 100) x 0.652 g
actual yield = 0.423 g
Therefore, the actual yield of the reaction was 0.423 g of CO2.
5. what will be the percent yield if 48 grams of iron is the actual yield ?
Answer:
Nasa picture ang answer
100% OK ^∆^
Brainliest po plss
6. Problem Solving Sample Problem Using the stoichiometry sample problem 2.a. Find the percent yield of iron (Fe) if the reaction was able to produce 45.82g Percent Yield Formula: Actual Yield (g) Theoretical Yield (g) x 100 45.82g Percent Yield of Fe = 55.96g Percent Yield of Fe = 81.88% - x 100 Practice Problem Use your answer in practice problem for stoichiometry. Find the percent yield of Na2SO4 if the actual yield is 62.42g. Is the reaction successful or not?
Answer:
To solve for the percent yield of Na2SO4, we need to know the actual and theoretical yields of the reaction. We can use stoichiometry to calculate the theoretical yield, and then use the percent yield formula to compute the percent yield.
Here is the balanced chemical equation for the reaction:
2 NaCl + H2SO4 → Na2SO4 + 2 HCl
From the balanced equation, we can see that 2 moles of NaCl react with 1 mole of H2SO4 to produce 1 mole of Na2SO4. Therefore, we can use the given mass of NaCl to calculate the theoretical yield of Na2SO4.
a. Calculate the theoretical yield of Na2SO4:
The molar mass of NaCl is 58.44 g/mol.
The mass of NaCl used in the reaction is not given in the problem, so let's assume it is 100 g for this example.
The molar mass of Na2SO4 is 142.04 g/mol.
From the balanced equation, 2 moles of NaCl react to produce 1 mole of Na2SO4.
Therefore, the number of moles of NaCl used in the reaction is: 100 g / 58.44 g/mol = 1.71 mol
The theoretical yield of Na2SO4 is: 1.71 mol NaCl x (1 mol Na2SO4 / 2 mol NaCl) x 142.04 g/mol Na2SO4 = 121.88 g
b. Calculate the percent yield of Na2SO4:
The actual yield of Na2SO4 is given as 62.42 g.
Using the formula for percent yield: Percent Yield = (Actual Yield / Theoretical Yield) x 100%
Substituting the given values: Percent Yield = (62.42 g / 121.88 g) x 100% = 51.16%
c. Determine whether the reaction was successful:
The percent yield of Na2SO4 is 51.16%.
A percent yield below 100% indicates that the actual yield is less than the theoretical yield, which could be due to experimental errors or incomplete reactions.
Therefore, the reaction was not completely successful, and there was a loss of product or reactants due to various reasons.
Explanation:
7. what is the difference between theoritical yield and actual yield
Answer:
The theoritical yield is the maximum posible mass of product that can be made from chemical reaction while the actual yield is what you actually get from a chemical reaction or the quantity of product found in chemical reaction.
I HOPE IT HELPS GUYS
8. Theoretically, the reaction can yield 88g of CO2. However, the actual yield is only 75g. What is the actual yield?
Answer:
71.7%
Explanation:
A reaction's percent yield essentially tells you many grams of a given product will actually be produced instead of a theoretical
100 g
of product.
Simply put, you can calculate a reaction's percent yield by dividing the actual yield, which is what the reaction actually produces, by the theoretical yield, which is what the reaction should theoretically produce, and multiplying the result by
100
.
9. DIRECTIONS: Solve the following problems. Write your answer on a short bond paper. A complete solution is required. 1. Calculate the percent yield of a reaction that had a theoretical yield of 3.76 g and an actual yield of 1.45 g. 2. If 2.5 g of K3PO4 was produced in the reaction below and the percent yield was 45%, what was the theoretical yield? 3KOH + H3PO4 ⟶ K3PO4 + 3H2O 3. If the actual yield of a reaction was 0.567 g, and the theoretical yield was 0.750 g, what was the percent yield of this reaction? 4. If the percent yield of a reaction was 65.0% and its theoretical yield was 0.652 g of CO2 what was the actual yield?
[tex]\tt{\huge{\red{1. \: Solution:}}}[/tex]
[tex]\begin{aligned} \text{percent yield} & = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100\% \\ & = \frac{\text{1.45 g}}{\text{3.76 g}} \times 100\% \\ & = \boxed{38.6\%} \end{aligned}[/tex]
Hence, the percent yield of the reaction is 38.6%.
[tex]\tt{\huge{\red{2. \: Solution:}}}[/tex]
[tex]\begin{aligned} \text{theoretical yield} & = \frac{100\%}{\text{percent yield}} \times \text{actual yield} \\ & = \frac{100\%}{45\%} \times \text{2.5 g} \\ & = \boxed{\text{5.6 g}} \end{aligned}[/tex]
Hence, the theoretical yield is 5.6 g.
[tex]\tt{\huge{\red{3. \: Solution:}}}[/tex]
[tex]\begin{aligned} \text{percent yield} & = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100\% \\ & = \frac{\text{0.567 g}}{\text{0.750 g}} \times 100\% \\ & = \boxed{75.6\%} \end{aligned}[/tex]
Hence, the percent yield of the reaction is 75.6%.
[tex]\tt{\huge{\red{2. \: Solution:}}}[/tex]
[tex]\begin{aligned} \text{actual yield} & = \frac{\text{percent yield}}{100\%} \times \text{theoretical yield} \\ & = \frac{65.0\%}{100\%} \times \text{0.652 g} \\ & = \boxed{\text{0.424 g}} \end{aligned}[/tex]
Hence, the actual yield is 0.424 g.
[tex]\\[/tex]
Note: Kindly swipe the screen to the left to see the continuation of the answers on the right side.[tex]\\[/tex]
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10. explain the concept of limiting reactant ,excess reactant ,theoretical yield actual yield and percent yield
Answer:
A limiting reagent is a chemical reactant that limits the amount of product that is formed.
11. difference between actual yield and theoretical yield
Answer:
The difference between actual yield and theoretical yield is the Theoretical yield is what you expect stoichiometrically from a chemical reaction; actual yield is what you actually get from a chemical reaction.
Explanation:
12. If the actual yield of C6H5Br is 63.6 g, what is the percent yield?
Explanation:
iyan lang po ang kaya ko sorry
13. What do terms “actual yield”, “theoretical yield”, and “percentage yield” mean? How are they related?
Answer:
Amounts of products calculated from the complete reaction of the limiting reagent are called theoretical yields, whereas the amount actually produced of a product is the actual yield. The ratio of actual yield to theoretical yield expressed in percentage is called the percentage yield.
Explanation:
Hope it helps
14. If the actual yield is 19.1g, what is the percent yield?
Answer:
the percent yield cannot be determined.
Explanation:
the percent yield cannot be determined without the theoretical yield. pero here's the formula in calculating the percent yield:
%yield = actual yield/theoretical yield * 100%
u can message me po if u need help in calculating the theoretical yield.
15. 1. Calculate the percent yield of a reaction that produced 0 350 mol Hat the theoretical yield was 15.36g. 2.Calculate the percent yield of a reaction that had a theoretical yield of 3.76 g and an actual yield of 1.45g.I NEED THE ANSWER PLEASE
Answer:
[tex]\small\ answer :[/tex]
btw, thanks sa po ints, have a nice day^_^
Explanation:
srry need ko lng po ng points :)
16. 1. input: 1800g output: 1100g yield= 2. input: 1480g output: 1100g yield= 3. input: 500g output: 250g yield= 4. input: 1200g output: 300g yield = 5. input: 2400g output: 400g yield =
Answer:
ano po ang gagawin
Explanation:
dyan huh
17. 2. The formula for getting the percentage yields is% Yield =
Answer:
%yield = (actual yield/theoretical yield) x 100.
18. The process of fermentation which yields ethanol also yields:
Ethanol fermentation, also called alcoholic fermentation, is a biological process which converts sugars such as glucose, fructose, and sucrose into cellular energy, producing ethanol and carbon dioxide as by-products.
19. In a particular experiment to prepare a compound, the theoretical yield is 34.7 g. If the actual yield is 31.2 g, what is the percent yield?
Answer:
percent yield = 89.9%
Explanation:
Calculating the percent yield
percent yield = (actual yield / theoretical yield) × 100
percent yield = (31.2 g / 34.7 g) × 100
percent yield = 89.9%
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20. Will things change if you yield/do not yield to social pressure?
Answer:
Yes,the outcome will always be different depending on how you assess it.
21. In a chemical reaction, what are the actual yield and percent yield?
Answer:
Amounts of products calculated from the complete reaction of the limiting reagent are called theoretical yields, whereas the amount actually produced of a product is the actual yield. The ratio of actual yield to theoretical yield expressed in percentage is called the percentage yield.
22. 3. the sum of squares of yield a number × and 3 yield 25
Answer:
Anwser it your self 8282
Step-by-step explanation:
9292829
23. if the percent yield for erection is 100% and the theoretical yield is 88 g what is the actual yield ?
Answer:
actual yield= 88g
Explanation:
kung tama, pa brainliest po. thank you
24. Actual yield cannot be greater than the theoretical yield.
Theoretical yield will never be higher than actual yield. Theoretical yield is the result if the reaction is 100% efficient and there are no impurities or errors during the experiment.
25. What is the importance of percent yield in obtaining theoretical and actual yield?
Answer:
The percentage yield of a chemical reaction is an important consideration in industrial chemistry. It can be calculated to compare the yield (quantity) of product actually obtained with what could have been obtained in theory, if all of the reactants were converted with no loss or waste.
Explanation:
pa brainliest
26. if the theoretical yield of ZnC12 is 150 grams but the actual yield is 123,5 grams, what is the percent yield of the reaction?
Answer:
If the theoretical yield of ZnC12 is 150 grams but the actual yield is 123
27. if the actual yield equals 15 g and the theoretical yields is 20 g, calculate the percent yield.
Answer:
pic po kelangan ko
Explanation:
para Makita kopo
28. Old Yield = 2 New Yield = 20 Conversion Factor = ?
Answer:conversion factor = 10%
Explanation:
For example, to convert inches to feet, the appropriate conversion value is 12 inches equal 1 foot. To convert minutes to hours, the appropriate conversion value is 60 minutes equal 1 hour
29. How to calculate the percentage yield? A. % Yields = production input x 100B. % Yields = production output x 100C. % Yields = production input /production output x 100D. % Yields = production output/production input x 100
Answer:
D. % Yields = production output/production input x 100
30. differentiate between theoretical yield and actual yield.
Answer:
Theoretical yield is what you calculate the yield will be using the balanced chemical reaction. Actual yield is what you actually get in a chemical reaction. Percent yield is a comparison of the actual yield with the theoretical yield.
