Problem 7.100 with feedback Clinical Application Part C Use your balanced chemic

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Problem 7.100 with feedback Clinical Application Part C Use your balanced chemical equation to calculate the number of moles of HF needed to react with 0.530 mole of SnO Express the number of moles to three significant figures. The reaction of hydrogen peroxide, H202( placed on Jane's teeth produces water, H20(1) and oxygen gas. and whitened, Kimberly recommended that she use a toothpaste with tin(II) fluoride when she brushes her teeth. Most toothpastes and mouthwashes contain fluoride ions. Tooth enamel, which is composed of hydroxyapatite, Cas (PO)3H, gthened when it reacts with fluoride ions to form fluoroapatite Cas(POs)3H After Jane had her teeth cleaned mol HF Submit My Answers Give Up You may want to reference (L..pages265-27 Section 7.8 while completing this problem. Use the balanced chemical equation to calculate the grams of HF that need to react with 4.22 g of SnF2 Express the mass in grams to three significant figures AZd g HF Submit My Answers Give Up Part E If 5.20 g of HF completely reacts, what is the theoretical yield of SnF2? Express the mass in grams to three significant figures. g SnF2 Submit My Answers Give Up

Explanation / Answer

Ans 7.118 :

Part A :

the balanced reaction is given as :

2Cl2 (g) + O2 (g) = 2Cl2O (g)

part B :

the picture in the products side shows , one molecule of oxygen gas left unused , which indicates that oxygen was in excess.

So the limiting reagent was Cl2 molecules.

Part C :

Pecent yield = ( actual yield / theoretical yield) x 100

3 molecules of O2 would produce 6Cl2O molecules theoretically

But actual yield = 4 molecules

So percent yield = ( 4/6) x 100

= 66.67 %

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