Yield and Error - AP Chemistry
Card 0 of 46
3 mols of 
are placed in a reactor and react to form 
as in the above reaction. At equilibrium, there are 1.75 mols of 
.
What is the percent conversion of 
?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of 
. We know that every 1 mol of 
that is consumed in the reaction yields 1 mol of 
. Therefore, the final amount of 
in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above
You run an experiment in order to empirically find the gas constant, 
. You find
You know from the literature that
What is the percent error in your experimental value of 
?
You run an experiment in order to empirically find the gas constant,
You know from the literature that
What is the percent error in your experimental value of
To find the percent error in your 
value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
To find the percent error in your
Doing this, we find the percent error to be 4.6%.
Compare your answer with the correct one above
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce 
of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that 
are produced. What is the percent yield of caffeine in this synthesis process?
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was 
efficient.
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was
Compare your answer with the correct one above
3 mols of are placed in a reactor and react to form as in the above reaction. At equilibrium, there are 1.75 mols of .
What is the percent conversion of ?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of . We know that every 1 mol of that is consumed in the reaction yields 1 mol of . Therefore, the final amount of in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above
You run an experiment in order to empirically find the gas constant, . You find
You know from the literature that
What is the percent error in your experimental value of ?
You run an experiment in order to empirically find the gas constant,
You know from the literature that
What is the percent error in your experimental value of
To find the percent error in your value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
To find the percent error in your
Doing this, we find the percent error to be 4.6%.
Compare your answer with the correct one above
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that are produced. What is the percent yield of caffeine in this synthesis process?
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was efficient.
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was
Compare your answer with the correct one above
3 mols of are placed in a reactor and react to form as in the above reaction. At equilibrium, there are 1.75 mols of .
What is the percent conversion of ?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of . We know that every 1 mol of that is consumed in the reaction yields 1 mol of . Therefore, the final amount of in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above
You run an experiment in order to empirically find the gas constant, . You find
You know from the literature that
What is the percent error in your experimental value of ?
You run an experiment in order to empirically find the gas constant,
You know from the literature that
What is the percent error in your experimental value of
To find the percent error in your value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
To find the percent error in your
Doing this, we find the percent error to be 4.6%.
Compare your answer with the correct one above
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that are produced. What is the percent yield of caffeine in this synthesis process?
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was efficient.
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was
Compare your answer with the correct one above
3 mols of are placed in a reactor and react to form as in the above reaction. At equilibrium, there are 1.75 mols of .
What is the percent conversion of ?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of . We know that every 1 mol of that is consumed in the reaction yields 1 mol of . Therefore, the final amount of in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above
You run an experiment in order to empirically find the gas constant, . You find
You know from the literature that
What is the percent error in your experimental value of ?
You run an experiment in order to empirically find the gas constant,
You know from the literature that
What is the percent error in your experimental value of
To find the percent error in your value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
To find the percent error in your
Doing this, we find the percent error to be 4.6%.
Compare your answer with the correct one above
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that are produced. What is the percent yield of caffeine in this synthesis process?
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was efficient.
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was
Compare your answer with the correct one above
3 mols of are placed in a reactor and react to form as in the above reaction. At equilibrium, there are 1.75 mols of .
What is the percent conversion of ?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of . We know that every 1 mol of that is consumed in the reaction yields 1 mol of . Therefore, the final amount of in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above
You run an experiment in order to empirically find the gas constant, . You find
You know from the literature that
What is the percent error in your experimental value of ?
You run an experiment in order to empirically find the gas constant,
You know from the literature that
What is the percent error in your experimental value of
To find the percent error in your value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
To find the percent error in your
Doing this, we find the percent error to be 4.6%.
Compare your answer with the correct one above
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that are produced. What is the percent yield of caffeine in this synthesis process?
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was efficient.
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was
Compare your answer with the correct one above
The literature value for the melting point of a given compound is 240 degrees Celsius. A scientist uses the melting point apparatus to experimentally measure the compound's melting point at 230 degrees Celsius. What is the scientist's percent error?
The literature value for the melting point of a given compound is 240 degrees Celsius. A scientist uses the melting point apparatus to experimentally measure the compound's melting point at 230 degrees Celsius. What is the scientist's percent error?
The percent error is given by the following formula:
In this case, the theoretical value is 240 degrees Celsius, and the actual value is 230 degrees Celsius. The percent error is thus calculated to be 4.16 %. The calculation is as follows:
The percent error is given by the following formula:
In this case, the theoretical value is 240 degrees Celsius, and the actual value is 230 degrees Celsius. The percent error is thus calculated to be 4.16 %. The calculation is as follows:
Compare your answer with the correct one above
3 mols of are placed in a reactor and react to form as in the above reaction. At equilibrium, there are 1.75 mols of .
What is the percent conversion of ?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of . We know that every 1 mol of that is consumed in the reaction yields 1 mol of . Therefore, the final amount of in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above
You run an experiment in order to empirically find the gas constant, . You find
You know from the literature that
What is the percent error in your experimental value of ?
You run an experiment in order to empirically find the gas constant,
You know from the literature that
What is the percent error in your experimental value of
To find the percent error in your value, you can use the following equation:
Doing this, we find the percent error to be 4.6%.
To find the percent error in your
Doing this, we find the percent error to be 4.6%.
Compare your answer with the correct one above
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce of caffeine. After the chemist finishes synthesizing the caffeine, he weighs it only to find out that are produced. What is the percent yield of caffeine in this synthesis process?
Suppose that a chemist working in a lab is trying to synthesize caffeine. In doing so, he predicts that he can produce
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was efficient.
When chemists synthesize compounds in the lab, a theoretical yield can be calculated by using knowledge of the full, balanced chemical equation, as well as the starting amounts of all reagents including the limiting reagent. However, due to a variety of factors, the actual yield obtained at the end of the experiment is nearly always going to be lower than the theoretical yield. Some of the things that can cause this are experimental error and side reactions, among others. Thus, chemists usually take the ratio of actual yield to theoretical yield to give the percent yield.
This means that the overall process was
Compare your answer with the correct one above
3 mols of are placed in a reactor and react to form as in the above reaction. At equilibrium, there are 1.75 mols of .
What is the percent conversion of ?
3 mols of
What is the percent conversion of
To find the percent conversion, use the following equation:
Initially there are 3 mols of . We know that every 1 mol of that is consumed in the reaction yields 1 mol of . Therefore, the final amount of in mols is
Plugging this into the above equation gives a conversion rate of 58%.
To find the percent conversion, use the following equation:
Initially there are 3 mols of
Plugging this into the above equation gives a conversion rate of 58%.
Compare your answer with the correct one above