Question

Air Oxidation of Fluorenone to 9-fluorene 1. Determine the limiting reagent (fluorene or sodium hydroxide) and...

Air Oxidation of Fluorenone to 9-fluorene 1. Determine the limiting reagent (fluorene or sodium hydroxide) and 2. Calculate percent yield.

Beginning mass of Fluorane: 0.8007g

End Mass of recrystalized 9-fluorenone by vacuum filtration: 0.423g

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
determine percent yield of each isomer. (the weight of the other isomer is the difference between...
determine percent yield of each isomer. (the weight of the other isomer is the difference between the mass of the product and the mass of the starting material..) we weighed out .2 g of maleic acid. added .3 ml of water and .25ml of HCL. then refluxed gently for 30mins. cooled and collected solid product by vacuum filtration using hirsch funnel then recrystallized using hot solvent and air dried. the only data i have taken down is mass starting material...
1. Solid lithium hydroxide is used to "scrub" CO2 from the air in spacecraft and submarines;...
1. Solid lithium hydroxide is used to "scrub" CO2 from the air in spacecraft and submarines; it reacts with the CO2 to produce lithium carbonate and water. What volume in liters of CO2 at 25°C and 715 torr can be removed by reaction with 405 g of lithium hydroxide? Enter to 3 sig figs. 2.The alkali metals react with the halogens to form ionic metal halides. What mass in g of sodium chloride forms when 6.00 L of chlorine gas...
A student determined the heat of neutralization of sulfuric acid mixed with sodium hydroxide solution using...
A student determined the heat of neutralization of sulfuric acid mixed with sodium hydroxide solution using the procedure described in this experiment. 35.0 mL of 1.00 M H2SO4 were added to 70.5 mL of 1.00 M NaOH solution. 1)Calculate the mass of the reaction mixture. Assume that the density of the mixture is 1.03 g/mL. _______g/mL 2)Calculate the number of moles of each reagent that are consumed when the solutions are mixed. Record your responses using decimal notation rather than...
1. A sample of hydrochloric acid is standardized using sodium bicarbonate. a. Write the balanced chemical...
1. A sample of hydrochloric acid is standardized using sodium bicarbonate. a. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bicarbonate, NaHCO3 b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. c. Calculate the mass percent concentration of hydrochloric acid using the molar concentration calculated in part b and assuming the density of the solution...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperature is 0.75 mol per liter. Also assume that all the sodium bicarbonate precipitated is collected and converted quantitatively to sodium carbonate The mass of sodium chloride in (g) is...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperature is 0.75 mol per liter. Also assume that all the sodium bicarbonate precipitated is collected and converted quantitatively to sodium carbonate The mass of sodium chloride in (g) is...
1) An air-standard Otto cycle has a compression ratio of 9. At the beginning of the...
1) An air-standard Otto cycle has a compression ratio of 9. At the beginning of the compression process, the temperature is 20°C, and the pressure is 100 kPa. The heat added is 500 kJ/kg. Determine the cycle efficiency, work output, and the heat rejected 2) An air-standard Otto cycle operates with a minimum temperature of 300 K and a maximum temperature of 1700 K. The compression ratio of the cycle is 7. At the beginning of the compression process, the...
Molarity: Determine the concentration of the following solutions. 1. 35 moles of sodium chloride dissolved in...
Molarity: Determine the concentration of the following solutions. 1. 35 moles of sodium chloride dissolved in a final volume of 9.5L will produce a sodium chloride solution with what concentration? 2. If you dissolve 12g of sodium hydroxide in a final volume of 5L, what is the concentration of the resulting solution? 3. If you dissolve 12g of sodium hydroxide in a final volume of 125ml, what is the concentration of the resulting soltuion? 4. If you dissolve 0.012 moles...
Skills Review: Titration Objective: Determine the concetration of an acid by mas percent and by molarity....
Skills Review: Titration Objective: Determine the concetration of an acid by mas percent and by molarity. Summary You will perform four titrations to brush up on titration skills. The analytes used in the experiment are commercial vinegar and hydrochloric acid. The titrant used for all titrations is sodium hydroxide. The indicators used to find the endpoint of the titrations are methyl red and phenolphthalein. Titrations #1-commerical vinegar and sodium hydroxide with methyl red indicator Titrations #2-commerical vinegar and sodium hydroxide...
1.Calculate the theoretical mass of sodium carbonate that should be produced by heating 1.678 g of...
1.Calculate the theoretical mass of sodium carbonate that should be produced by heating 1.678 g of sodium bicarbonate. 2.If 1.018 grams of sodium carbonate were produced from the sodium bicarbonate in question 1, calculate the percent yield for the bicarbonate decomposition reaction. 3.A classic high school lab experiment involves combining a solution of barium nitrate, Ba(NO3)2, with a sodium sulfate solution, Na2SO4, forming a precipitate of barium sulfate. Ba(NO3)2(aq) + Na2SO4(aq) ---> BaSO4(s) + 2NaNO3(aq) a. Identify the hazards associated...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT