Stoichiometry Part 2b: moles to mass. What mass of carbon dioxide, in grams, is needed to react 3.00...
-
Upload
austin-holt -
Category
Documents
-
view
219 -
download
1
Transcript of Stoichiometry Part 2b: moles to mass. What mass of carbon dioxide, in grams, is needed to react 3.00...
StoichiometryPart 2b: moles to mass
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g)
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol)
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1:
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6)
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2:
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2)
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol)
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) ?
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) 132 g
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g
1
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) 132 g
n (mol) 3.00 3.00
2
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?
Ṃ (g/mol) 44.0 18.0 180.2 32.0
6 CO2(g) + 6 H2O(l) →C6H12O6(s) + 6 O2(g)
m (g) 132 g
n (mol) 3.00 3.00
Step 1: Find the number of moles of CO2 used in the reaction.nCO2/nH2O = coeffCO2/coeffH2O
nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 molStep 2: Find the mass of the CO2 used in the reaction.
mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g
What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?