A few days ago
Chemistry Homework Question, Please Help; Regards Net Ionics and Empirical Formulas?
A student was given 2.982 grams of a test tube sample of a pure anhydrous Compound A, made up of elements lead and chlorine. The student added a small amount of water to the test tube and heated it in a fume hood, liberating chlorine gas and creating Compound B. A flask filled with 0.5 M (molar solution) NaOH helped trap the chlorine gas. The student then heated Compound B, driving off the remaining water, and determined the mass of Compound B as 2.364 grams. The student then reduced Compound B with hydrogen gas to form elemental lead. The chlorine in Compound B was drive off as HCL (g). This lead was massed and found to weigh 1.770 grams.
a) What is the Empirical Formula of Compound B?
b) What is the Empirical Formula of Compound A?
c) Write the balanced chemical equations and the net ionic equations involved in generating Compound B and elemental lead.
*Instead of just telling me what the answer is, please tell me how you got there! Thanks!!!*
Top 3 Answers
A few days ago
Favorite Answer
Isolate the weight of each of the elements. For example, you know that in Comp B, 1.770 is Pb, and the rest, 2.364-1.770, is Cl. So, knowing the weight, find how mane MOLES of each there are, and what their ratio is for question (a). So, if you find there is .3 Pb to each .5 Cl, multiply them to lowest integers, and use as subscripts. (Those are random number for illustation purposes only.)
Use similar approach to solve part (b).
For part (c)… oh dear. Sorry, this was a year ago, I’m afraid I’m a bit rusty! Good luck, though.
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A few days ago
Okay I would really like to help but I am a bit rusty with my chemistry, especially those involving calculations :). Why don’t you get help from the experts. Try http://www.tuitionplaza.com/tutoring/homework_help.asp – homework help by retired teachers and volunteers (free)
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A few days ago
A THERES NO WAY TO EXPLAIN It
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