Question

Consider again the reaction for photosynthesis: 6CO2 + 6H2O â C6H12O6 + 6O2 What mass of water is required to react completely with 157.35 g CO2? (Molar mass of H2O = 18.02 g/mol; molar mass of CO2 = 44.01 g/mol)

Answer 1

We Need 18.02*157.35/44.01=64.43 g h2o

Answer 2

Answer: 64.9 g

Explanation:

Moles is calculated by using the formula:

$Moles=\frac{\text{Given mass}}{\text{Molar mass}}$

${\text {moles of}CO_2}=\frac{157.35g}{44.01g/mol}=3.6moles$

$6CO_2+6H_2O\rightarrow C_6H_{12}O_6+6O_2$

As can be seen from the balanced chemical equation,

6 moles of carbon dioxide $(CO_2)$ combines with 6 moles of water $(H_2O)$.

Thus 3.6 moles of carbon dioxide $(CO_2)$ combines with 3.6 moles of water $(H_2O)$.

${\text {mass of water}}={\text {number of moles}}\times {\text {molar mass}}$

${\text {mass of water}}={3.6moles}\times {18.02g/mol}=64.9g$

64.9 g of water is required to react completely with 157.35 g $CO_2$.