Determining the Formula of a Compound

bearblondi · Probably a bot. Joined: 05 Dec 2005 Posts: 1

I need some serious help.. I have a Formula of a Compound problem set and I can't figure out how to do some problems (my brain is fried) Could anyone help out? Any type of information will be most appreciated.

1.

Calculate the mass of zinc chloride produced. You know the original mass of the beaker. You also know the mass of the beaker plus the product you produced, which is zinc chloride. The difference between these two masses is the mass of zinc chlorine produced. Subtract the original mass of the beaker from the mass of the beaker plus the zinc chloride produced. Show your work.
Formula:
(mass beaker + zinc chloride) - mass of beaker = mass of zinc chloride produced
( 55.45 + 30 ) - 55.45 = 30

2.
Calculate mass of chlorine reacted. To do this, you know that the zinc and the hydrochloric acid combined to create zinc chloride. You know the mass of zinc used, and the mass of zinc chloride produced; so, the difference (subtract) between these values is the mass of chlorine reacted.
Formula:
Mass of zinc chloride produced - mass of zinc used = mass of chloride reacted.
30 - 1.80 = 28.2

3.
Calculate moles of zinc based on original mass of zinc. Show your calculations.
Formula:

4.
Calculate moles of chlorine reacted based on your answer for #2. Show your work.
Formula:

5.
What is the experimental empirical formula of zinc chloride? Determine the simplest whole number ratio of moles of zinc used, to moles of chlorine reacted in the zinc chloride that was produced. (Take your answers to #4 and #5, and divide both values by whatever value is smaller.)

6.
Determine the actual empirical formula of zinc chloride, based on the ionic charges of zinc and chloride ions, using your rules for ionic nomenclature.

7.
Does your experimental empirical formula (answer to #6.) agree with the known empirical formula (answer to #7.) of zinc chloride? List and describe some sources of error that may have affected your results.