1. Stoichiometry pd 5 3/25/10

2. #20 What mass of K 2 O is produced when 6.92 g of K reacts with 4.28 g of O 2 ?

3. First Step Balance equation Make an equation Start Making Ratios

4. Incorrect *Remember you can’t start the ratio without an equation Back to the question

5. Step #2 Which is the correct equation? K + O 2 K 2 O 4K + O 2K 2 O 4K + O 2 2K 2 O

6. Correct To the next step

7. Correct To the next step

8. Correct To the next step

9. Correct To the next step

10. Correct To the next step

11. Correct To the next step

12. Correct To the next step

13. Correct YOU FINISHED THE EQUATION

14. Incorrect Back the question Remember Balance the equation

15. Step #3 Which one is the correct ratio setup? Here is the original question and the balanced Equation. What mass of K 2 O is produced when 6.92 g of K reacts with 4.28 g of O 2 ? 4K + O 2 2K 2 O

16. Incorrect Make sure you cancel out your elements. Make sure you have the right numbers in the right places. Back to the question

17. Step #4 What is the answer? 2.4 g K 2 O 8.34 g K 2 O 8.34 g O 2

18. Incorrect Make sure you multiply not add Back to the question

19. Step #5 What about the other element? What is the setup for the next ratio? Here is the original Problem and the balanced equation.  What mass of K 2 O is produced when 6.92 g of K reacts with 4.28 g of O 2 ?  4K + O 2 2K 2 O

20. Incorrect Make sure your compounds are opposite of each other Back to the question

21. Step #6 What is the answer? 25.2 g K 2 O 25.2 g O 2 4.28 g K 2 O

22. Incorrect Make sure you have the correct unit/compound and make sure you multiplied right Back to the question

23. Step #7 Limiting Reactants How do you tell which one is the limiting reactant? Which ever one is the lesser one Which ever one is more than the other I do not know

24. Incorrect Limiting is the key word, it usually means less Back to the question

25. Step #8 Which one is limiting? 8.34 g K 2 0 25.2 g K 2 O None

26. Incorrect Limiting = less Back to the Question

27. The End