Describe the appearance of your gas chromatogram; was there just one peak, or multiple peaks? If more than one peak was present, why do you think that is? 2. Compare your gas chromatogram with those collected for the different types of fruit. What peaks do these different citrus fruits have in common? What are the differences? 3. Look at the collected online data for your lab section and the entire class. For your section, what is the average amount of limonene for each fruit based on your classmates’ calculations? Is the amount of limonene consistent for each type of fruit? List some experimental reasons why the amounts may not be consistent. 4. Go online or to the Chemistry Library (see the Introduction/Table of Physical Constants for information on sources of chemical information) and look up the solubility of limonene in different solvents. Would water be a good solvent to extract limonene from citrus peels? Why or why not?

100mg magnesium reacts with 20ml of 1.0m hcl

In this chemical reaction, 325 grams of barium (ba) react completely. how many moles of lithium (li) are produced?

Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, pbutane, alone. to do this, consult a reference and record the partial pressure of the water vapor, pwater, at the temperature you recorded. use the following formula to compute the partial pressure of the butane. pbutane = atmosphere - pwater use the following combined gas law formula and compute the volume that the butane sample will occupy at stp. (hint: convert both temperatures to kelvin.) pbutane x voriginal = pstandard x vfinal troom tstandard use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. grams of butane you used “x” grams of butane ml of butane corrected to stp = 22,400 ml compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table. compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula: % error = measured value - accepted value x 100 accepted value use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. need asap