# Stoichiometry Part 2b: moles to mass. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described.

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Stoichiometry Part 2b: moles to mass

What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g) What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol) What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) = (3.00 mol)(44.0 g/mol) 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) = (3.00 mol)(44.0 g/mol) = 132 g 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) = (3.00 mol)(44.0 g/mol) = 132 g 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)? n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) = (3.00 mol)(44.0 g/mol) = 132 g 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)132 g n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) = (3.00 mol)(44.0 g/mol) = 132 g 1 (g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)132 g n (mol)3.003.00 2 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

(g/mol) 44.0 18.0 180.2 32.0 6CO 2 (g)+6H 2 O(l) C 6 H 12 O 6 (s)+6O 2 (g) m (g)132 g n (mol)3.003.00 Step 1: Find the number of moles of CO 2 used in the reaction. n CO2 /n H2O = coeff CO2 /coeff H2O n CO2 = (n H2O )(coeff CO2 )/coeff H2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO 2 used in the reaction. m CO2 = (n CO2 )( CO2 ) = (3.00 mol)(44.0 g/mol) = 132 g What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H 2 O in the photosynthetic reaction described in the previous problem?

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