Question

For the following reaction, the starting material weighs 3.00 grams and the final product weighs 2.00...

For the following reaction, the starting material weighs 3.00 grams and the final product weighs 2.00 grams. what is the percent yield for this reaction?

Cyclohexanol -----> cyclohexene + h2o

cyclohexanol molar mass: 100 grams

cyclohexene molar mass: 82 grams

Homework Answers

Answer #1

ANSWER:

The given reaction is:

Cyclohexanol Cyclohexene + H2O

Mass of cyclohexanol = 3.00 g

Mass of cyclohexene = 2.00 g

molar mass of cyclohexanol = 100 g

molar mass of cyclohexene = 82 g

Number of moles of reactant (cyclohexanol) = (mass)/(molar mass)

= (3.00)/(100)

= 0.03 moles

For the given reaction, one moles of reactant will give one mole of product. Since, number of moles of reactant is 0.03 moles so, number of moles of product will be 0.03 moles also by the theoritical calculation.

Theoritical mass of product = number of moles x molar mass

= 0.03 moles x 82 g/mol

= 2.46 g

And, given mass of product is 2.00 grams. So,

Percentage yield = (given mass x 100)/(theoritical mas)

= (2.00 g x 100)/(2.46 g)

= 81.30 %

Hence, the percent yield for this reaction is 81.30 %.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
If a reaction has 1 mole of a starting compound with 0.4969 grams of starting material,...
If a reaction has 1 mole of a starting compound with 0.4969 grams of starting material, and reacts to give 1 mole of product, what is the theoretical yield in grams? The starting compound molecular weight is 147.4 g/mol, and the product molecular weight is 121.4 g/mol.
Data: 8.0 grams of CuSO4 • 5H2O in a 125 mL Erlenmeyer flask: 8.130 grams 1)...
Data: 8.0 grams of CuSO4 • 5H2O in a 125 mL Erlenmeyer flask: 8.130 grams 1) Calculate the theoretical yield of Cu(NH3)4SO4 x H2O (Molecular Weight= 245.7 g/mol) from the mass of the starting material, CuSO4 x 5H2O (Molecular Weight= 249.7 g/mol) 2) Calculate the percent yield of the product. ( experimental yield/theoretical yield ) x 100 3) Calculate the theoretical percents of copper, ammonia, sulfate and water from the formula, Cu(NH3)4SO4 x H2O
Q.1 Given a reaction where 1 mole of starting compound reacts to give one mole of...
Q.1 Given a reaction where 1 mole of starting compound reacts to give one mole of product, what is the theoretical yield in grams if you start with 0.1517 grams of the starting material? Starting Compound Molecular Weight: 75.8 g/mol Product Molecular Weight: 127.3 g/mol Round your number to 4 significant digits. The unit is not required. Q.2 If one mole of starting compounds reacts to give one mole of product, what is the percent yield of the product if...
LIMITING REAGENT PROBLEM: Show your work! PLEASE MAKE SURE IT IS CLEAR HOW THE MOLES OF...
LIMITING REAGENT PROBLEM: Show your work! PLEASE MAKE SURE IT IS CLEAR HOW THE MOLES OF Ba3(PO4)2 and NaNO3 are found and be descriptive with the entire process. Consider the reaction and complete the following table: 2 Na3PO4 + 3 Ba(NO3)2 ----> Ba3(PO4)2 + 6 NaNO3 Initial Mass 100.0grams 100.0grams ----------------- ----------- Change in Mass…. Amount used or formed Final mass Molar Masses: Na3PO4 = 164 grams/mole Ba(NO3)2 = 261 grams/mole Ba3(PO4)2 = 602 grams/mole NaNO3 = 85 grams/mole b)...
3. Answer the following with this reaction: P4O10+6PCl5 = 10POCl3 a. How many grams of POCl3...
3. Answer the following with this reaction: P4O10+6PCl5 = 10POCl3 a. How many grams of POCl3 are produced when 225.0 grams of P4O10 and 675.0 grams of PCl5 react? b. How many grams of excess reactant remain after the reaction in (a)? c. When 42.66 grams of PCl5 react with excess P4O10, the amount of product formed is 47.22 grams of POCl3. What is the percent yield?
For the following reaction, 4.49 grams of chlorine gas are mixed with excess iron . The...
For the following reaction, 4.49 grams of chlorine gas are mixed with excess iron . The reaction yields 5.06 grams of iron(III) chloride . iron ( s ) + chlorine ( g ) iron(III) chloride ( s ). What is the theoretical yield of iron(III) chloride in grams? What is the percent yield for this reaction?
For the following reaction, 3.35 grams of sulfur dioxide are mixed with excess oxygen gas ....
For the following reaction, 3.35 grams of sulfur dioxide are mixed with excess oxygen gas . The reaction yields 2.83 grams of sulfur trioxide . sulfur dioxide ( g ) + oxygen ( g ) sulfur trioxide ( g ) What is the theoretical yield of sulfur trioxide ? grams What is the percent yield for this reaction ? %
For the following reaction, 6.72 grams of carbon (graphite) are mixed with excess oxygen gas ....
For the following reaction, 6.72 grams of carbon (graphite) are mixed with excess oxygen gas . The reaction yields 19.7 grams of carbon dioxide . carbon (graphite)(s) + oxygen(g) carbon dioxide(g) What is the ideal yield of carbon dioxide? grams What is the percent yield for this reaction? %
1: If 30.4 g of H2S is reacted with 30. 4 g of SO2 in the...
1: If 30.4 g of H2S is reacted with 30. 4 g of SO2 in the following balanced reaction, which species is the limiting reactant? 2 H2S + SO2  ⟶   2 H2O + 3 S The molar mass of H2S is 34.082 g/mol and the molar mass of  SO2 is 64.065 g/mol. A: SO2 B: S C: H2O D: There is none. E: H2s 2: John was sloppy when doing an experiment in the lab. His actual yield of product for a...
In calculating the percent yield for this experiment, which of following the statements is/are correct? a....
In calculating the percent yield for this experiment, which of following the statements is/are correct? a. In this unique case we can compare grams to grams since our molecular formula is the same and our mole ratio is 1:1. b. The mole ratio between Maleic and Fumaric Acid is 1:1. c. Just like any percent yield calculation you need to compare grams starting material to grams product. d. Just like any percent yield calculation we can use the balanced equation...