1. Why is it the LAW of CONSERVATION OF MATTER or MASS?

2. Conservation of matter (mass)

3. We all know the basic LAW of CONSERVATION of MATTER….

4. NEW SUBSTANCES are REFORMED from the SAME OLD ATOMS!
2 H2O  2 H2 + O2

5. NEW SUBSTANCES are REFORMED from the SAME OLD ATOMS!
2 H2O  2 H2 + O2
the LAW of
CONSERVATION
of MATTER

6. In a chemical reaction matter is neither created NOR destroyed.

7. In a chemical reaction, MATTER is NOT CREATED NOR DESTROYED.

8. In chemical reactions, MATTER is NOT CREATED nor DESTROYED
In chemical reactions, MATTER is NOT CREATED nor DESTROYED. The same atoms are just REARRANGED into NEW MOLECULES.
2 H2O  2 H2 + O2 2 CH2 + 3 O2  2 CO2 + 2 H2O 6 CO2 + 6 H2O  C6H12O6 + 6 O2

9. Everything balances out in the end...
Can you tell me which chemical reaction below BEST represents photosynthesis?

10. Everything balances out in the end...
Can you tell me which CHEMICAL REACTION below BEST represents photosynthesis?
WHY???

11. In chemical reactions, MATTER is NOT CREATED nor DESTROYED
In chemical reactions, MATTER is NOT CREATED nor DESTROYED. The same atoms are just REARRANGED into NEW MOLECULES.
2 H2O  2 H2 + O2
2 CH2 + 3 O2  2 CO2 + 2 H2O
6 CO2 + 6 H2O  C6H12O6  +  6 O2

12. CH4 + O2  CO2 + H2O Which TWO below should be added above
so that REACTANTS = PRODUCTS?

13. CH4 + 2 O2  CO2 + 2 H2O Which two below should be added above
so that REACTANTS = PRODUCTS?

14. FINISH EZ COEFFIECIENTS TO BALANCE….

15. Why is it the LAW of CONSERVATION OF MATTER or MASS?

16. WE GOT ___ REACTANTS TURNING INTO ONE PRODUCT HERE.
REACTIONS make NEW PRODUCTS from old reactants. REMEMBER!!! MATTER IS NOT CREATED NOR DESTROYED in a CHEMICAL REACTION!!!!
WE GOT ___ REACTANTS TURNING INTO ONE PRODUCT HERE.

17. REACTIONS make NEW PRODUCTS from old reactants. REMEMBER
REACTIONS make NEW PRODUCTS from old reactants. REMEMBER!!! MATTER IS NOT CREATED NOR DESTROYED in a CHEMICAL REACTION!!!!
WE GOT 2 REACTANTS TURNING INTO ONE PRODUCT HERE. Same atoms are CONSERVED on both sides.

18. Same MATTER (atoms) are CONSERVED on both sides.
So, if our 2 REACTANTS have a total MASS of 10 pounds, how many pounds of PRODUCT MUST we have?
Same MATTER (atoms) are CONSERVED on both sides.
10 lbs.

19. Same MASS is CONSERVED on both sides!
So, if our 2 REACTANTS have a MASS of 10 pounds, the PRODUCT must have a MASS of 10 pounds.
Same MATTER (atoms) are CONSERVED on both sides.
Same MASS is CONSERVED on both sides!
10 lbs.
10 lbs.

20. Same MASS is CONSERVED on both sides!
So, if our 2 REACTANTS have a MASS of 10 pounds, the PRODUCT must have a MASS of 10 pounds.
Same MATTER (atoms) are CONSERVED on both sides.
Same MASS is CONSERVED on both sides!
MATTER IS NEITHER
CREATED NOR DESTROYED
10 lbs.
10 lbs.

21. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
What if you start with 8 pounds of calcium reactant and you end up with 10 pounds of total product…
TOTAL REACTANT MASS = TOTAL PRODUCT MASS
8 lbs.
10 lbs.

22. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
What if you start with 8 pounds of calcium reactant and you end up with 10 pounds of total product…How much oxygen did you need for this reaction?
TOTAL REACTANT MASS = TOTAL PRODUCT MASS
8 lbs.
???
10 lbs.

23. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
What if you start with 8 pounds of calcium reactant and you end up with 10 pounds of total product…How much oxygen did you need for this reaction? 2 POUNDS!
TOTAL REACTANT MASS = TOTAL PRODUCT MASS
8 lbs.
2 lbs!!!
10 lbs.

24. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
What if you start with 12 pounds of calcium reactant and you add 4 pounds of oxygen, how much product is made?
TOTAL REACTANT MASS = TOTAL PRODUCT MASS
12 lbs.
4 lbs.
??? lbs.

25. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
What if you start with 12 pounds of calcium reactant and you end up with 4 pounds of oxygen, how much product is made? 16 POUNDS!
TOTAL REACTANT MASS = TOTAL PRODUCT MASS
12 lbs.
4 lbs.
16 lbs.

26. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
WHAT IF WE STARTED WITH 20 mL of HYDROGEN PEROXIDE (H2O2)
20 mL

27. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
WHAT IF WE STARTED WITH 20 mL of HYDROGEN PEROXIDE (H2O2) and MADE 16 mL of WATER.
20 mL
16 mL

28. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
WHAT IF WE STARTED WITH 20 mL of HYDROGEN PEROXIDE (H2O2) and MADE 16 mL of WATER.
HOW MUCH OXYGEN GAS IS PRODUCED?
20 mL
16 mL
??? mL

29. TOTAL REACTANT MASS = TOTAL PRODUCT MASS
WHAT IF WE STARTED WITH 20 mL of HYDROGEN PEROXIDE (H2O2) and MADE 16 mL of WATER.
HOW MUCH OXYGEN GAS IS PRODUCED? 4 mL!
20 mL
16 mL
4 mL!!!

30. How much oxygen gas do you need when you produce 14 grams of product from 11 grams of methane (CH4)?

31. How much oxygen gas do you need when you produce 14 grams of product from 11 grams of methane (CH4)?
11 g ???? = grams total

32. How much oxygen gas do you need when you produce 14 grams of product from 11 grams of methane (CH4)?
11 g g = grams total

33. How much carbon dioxide gas would be made from 32 mL of methane (CH4) & 12 mL of oxygen gas if you ended up with 24 mL of water?

34. How much carbon dioxide gas would be made from 32 mL of methane (CH4) & 12 mL of oxygen gas if you ended up with 24 mL of water?
32 mL mL = ???? mL
CONSERVATION of MASS IS EASY, you just solve the equation
for the missing variable!

35. How much carbon dioxide gas would be made from 32 mL of methane (CH4) & 12 mL of oxygen gas if you ended up with 24 mL of water? 20 mL!!!
32 mL mL = mL mL
CONSERVATION of MASS is EASY, you just solve the equation
for the missing variable!

36. Quiz/worksheet

37. conserv of matter lab