Question

The chemical equation below shows the photosynthesis reaction. 6CO2 + 6H2O mc010-1.jpg C6H12O6 + 6O2 The molar mass of carbon dioxide (CO2) is 44.01 g/mol. The molar mass of water (H2O) is 18.01 g/mol. A reaction uses 528 g of CO2. How many moles of water are used in this reaction?

Answer 1

Given:
6CO2 + 6H2O -> C6H12O6 + 6O2
molar mass of carbon dioxide (CO2) is 44.01 g/mol
molar mass of water (H2O) is 18.01 g/mol
528 g of CO2

Required:
moles of water

Solution:

528 g of CO2/ (44.01 g/mol CO2) = 12 moles CO2

12 moles CO2 (6 moles H2O/ 6 moles CO2) = 12 moles H2O

12 moles H2O (18.01 g/mol H2O) = 216.12 grams H2O

Answer 2

12 mol of water

Step-by-step explanation:

`6CO_2 + 6H_2O \longrightarrow C_6H_(12)O_6 + 6O_2`

First we must find the moles of CO2.

We know that 1 mole of co2 has a mass of 4.01 g so how many moles will there be in 528 g.

We apply a simple rule of three

`44.01 g CO_2\longrightarrow 1 mol CO_2\\ 528 g CO_2\longrightarrow x\\x= 528/44.01\\x=12 molCO_2`

By stoichiometry we know that for every 6 moles of carbon dioxide 6 moles of water are needed, now if we have 12 moles of carbon dioxide how many moles of water will be needed

We apply a simple rule of three

`6 molCO_2 \longrightarrow 6 mol H_2O\\ 12 mol CO_2 \longrightarrow x\\x= ((12).(6))/(6)\\ x= 12 mol H_2O`