Answered

Explore Westonci.ca, the leading Q&A site where experts provide accurate and helpful answers to all your questions. Get quick and reliable solutions to your questions from knowledgeable professionals on our comprehensive Q&A platform. Get quick and reliable solutions to your questions from a community of experienced experts on our platform.

34 g of O2 are reacted with excess Cs, causing a production of 199 g of Cs2O. What is the percent yield of this
reaction?
2 Cs + O2 ---> Cs2O

Sagot :

maacastrobr

Answer:

33.23 %

Explanation:

  • 4 Cs + O₂ → 2Cs₂O

First we convert 34 g of O₂ into moles, using its molar mass:

  • 34 g O₂ ÷ 32 g/mol = 1.0625 mol O₂

Then we convert O₂ moles into Cs₂O moles, using the stoichiometric coefficients of the balanced reaction:

  • 1.0625 mol O₂ * [tex]\frac{2molCs_2O}{1molO_2}[/tex] = 2.125 mol Cs₂O

Now we convert 2.125 moles of Cs₂O into grams, using its molar mass:

  • 2.125 mol Cs₂O * 281.81 g/mol = 598.85 g Cs₂O

598.85 g is the theoretical yield. Finally we proceed to calculate the percent yield:

  • 199 / 598.85 * 100% = 33.23 %
Thanks for using our platform. We're always here to provide accurate and up-to-date answers to all your queries. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.