Consider the photosynthesis reaction: 6 CO2(g) + 6 H2O(l) → 6 O2(g) + C6H12O6(aq) Which of following solution maps is used to find how many grams of glucose (C6H12O6) can be synthesized from 58.5 g of carbon dioxide (CO2)? Assume that there is enough water present to react with all of the carbon dioxide. g CO2 → mol C6H12O6 → g C6H12O6
g CO2 → mol CO2 → g C6H12O6
g CO2 → mol H2O → mol C6H12O6 → g C6H12O6
g CO2 → mol CO2 → mol C6H12O6 → g C6H12O6

The answer is g CO2 → mol CO2 → mol C6H12O6 → g C6H12O6

Explanation:

The balanced equation (ignoring the state symbols) for this reaction is:

6 CO2 + 6 H2O → 6 O2 + C6H12O6

Which means 6 moles of CO2 produce 1 mole of C6H12O6

58.5g of CO2 would then produce 1.33 mole of C6H12O6

(∵mass ÷ molar mass of CO2)

⇒0.22159 moles of C6H12O6 was produced by 58.5g of CO2 during reaction

0.22159 moles of C6H12O6 has 39.9g of C6H12O6

(numb of mol × molar mass of C6H12O6 = mass)

Hence the solution map for finding the mass of glucose produced is:

g CO2 → mol CO2 → mol C6H12O6 → g C6H12O6