In a laboratory experiment, a student calculated a experimental value of 15.60 grams coupled with 35.5 % error. Calculate the theoretical value from this laboratory experiment.
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In a laboratory experiment, a student calculated a experimental value of 15.60 grams coupled with 35.5...
Calculate the % error if a student completes the molar mass of ethanol experiment and determine the molar mass to be 49.19 g/mol when the actual molar mass of ethanol is 46.07 g/mol. (show your work) % error = |Experimental value - Actual value|/ Actual value x 100.
A student prepared aspirin (C9H8O4) in a laboratory experiment using the following reaction. C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 The student reacted 1.50 g salicylic acid (C7H6O3) with 2.00 g acetic anhydride (C4H6O3). The yield was 1.50 g aspirin. Calculate the theoretical yield and the percent yield for this experiment. theoretical yield
1. In the laboratory a student finds that it takes 81.6 Joules to increase the temperature of 14.1 grams of solid iodine from 25.0 to 39.4 degrees Celsius. The specific heat of iodine calculated from her data is J/g°C. 2. In the laboratory a student finds that it takes 116 Joules to increase the temperature of 11.8 grams of solid sulfur from 24.0 to 38.1 degrees Celsius. The specific heat of sulfur calculated from her data is J/g°C. 5.1
Post lab Questions: 1. While performing the formula of hydrate laboratory experiment, the lid accidently slips over the crucible to completely seal the crucible. a. What effect this change will cause on your calculated experimental results? Explain. b. Would your calculated percent water of hydration be high, low or unaffected? Explain your answer. 2. A student was asked to identify a sample of unknown hydrate. Student was provided with the following experimental data. 3.51 g sample of the hydrate when...
In the laboratory, a general chemistry student measured the pH of a 0.430 M aqueous solution of acetie acid to be 2.571. Use the information she obtained to determine the K, for this acid. Ka(experiment)- Submit Answer Retry Entire Group 9 more group attempts remaining In the laboratory a student measures the percent ionization of a 0.430 M solution of acetic acid to be 0626 %. Calculate value of Ka from this experimental data. Ka-l In the laboratory, a general...
2. Based on your experimental data cal KAl(SO4)2.nH20. in your experimental data calculated the value of n in the chemical formula 3. Calculate the theoretical percentage of SO2- in pure KAl(SO4)2.nH2O using a periodic table for atomic weights and the correct literature value for n. 4. Is your sample alum? Use the results of the three tests to support your answer. Discuss the accuracy of your tests and possible sources of experimental error. Mass of crucible and cover (9) s...
Indicate whether the following experimental mistakes will increase or decrease the calculated value of R; explain your answers. a.) In adjusting the final water level after the O2 was produced, the student adjusted the levels to the bottom of the water in the beaker and the top of the water in the flask (rather than correctly the top of each). b.) A student completed the experiment without waiting for the test tube to cool after heating.
1.) in the laboratory, a student measures the percent ionization of a 0.463 M solution of acetylsalicylic acid (aspirin), HC9H7O4, to be 2.46%. Calculate the value of Ka from this experimental data. Ka = ???? 2.) Calculate the percent ionization of a 0.419 M solution of hydrofluoric acid. % ionization = ???? % 3.) in the laboratory, a student measures the percent ionization of a 0.463 M solution of phenol (a weak acid), C6H5OH, to be 1.51 x 10^-3%. Calculate...
subject: calorimetry
Post Laboratory Questions 1. A student places 138 g of an unknown metal at 99.9°C into 60.00 g of water at 22.2 °C. The entire system reaches a uniform temperature of 31.5 °C. Calculate the specific heat capacity of the metal. 2. If the correct specific heat of the metal in problem 1 is 0.25 J/gºC, calculate the percent crror. 3. While transferring the piece of unknown metal to the calorimeter, the student dropped the metal into the...