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?