1. Stoichiometry volume -to- volume:

2. Stoichiometry volume -to- volume:
1) Determine the volume of CO2 produced when
78.4 L of C2H2 burns at STP.
2 C2H2(g) + 5 O2(g) → 4 CO2(g) H2O(g)

3. Stoichiometry volume -to- volume:
1) Determine the volume of CO2 produced when
78.4 L of C2H2 burns at STP.
2 C2H2(g) + 5 O2(g) → 4 CO2(g) H2O(g)
78.4 L
? L
4(22.4)L
2(22.4)L =
157 L CO2
X = =
Does it make sense?

4. Stoichiometry mass- to- volume:

5. Stoichiometry mass- to- volume:
Calculate the volume of ammonia produced when 42 g of dinitrogen gas react with dihydrogen gas at STP.
N2(g) + 3 H2(g) NH3(g)
catalyst

6. Stoichiometry mass- to- volume:
Calculate the volume of ammonia produced when 42.0 g of dinitrogen gas react with dihydrogen gas at STP.
N2(g) + 3 H2(g) NH3(g)
42.0 g
? L
catalyst
2(22.4) L
28.02 g =
67.2 L NH3
X = =
Does it make sense?

7. Stoichiometry mass- to- # of particles:

8. Stoichiometry mass- to- # of particles:
How many molecules of oxygen are produced when 29.2 g of water is decomposed by electrolysis according to this balanced equation?
2H2O(l) H2(g) + O2(g)
electricity

9. Stoichiometry mass- to- # of particles:
How many molecules of oxygen are produced when 29.2 g of water is decomposed by electrolysis according to this balanced equation?
2H2O(l) H2(g) + O2(g)
29.2 g
? molecules
electricity
36.04 g
6.02 x 1023 molec. =
X = =
4.88 x 1023 molec.
Does it make sense?