To calculate the amount of H2O and C3H6 that can be formed from 6 C3H8O, we need to know the balanced chemical equation for the reaction. The balanced chemical equation for the combustion of C3H8O is:

2C3H8O + 9O2 -> 6CO2 + 8H2O

From the balanced chemical equation, we can see that for every 2 moles of C3H8O that react, 8 moles of H2O are produced. Therefore, 6 moles of C3H8O will produce 6 * 8 = 48 moles of H2O.

The molar mass of H2O is 18 g/mol. Therefore, 48 moles of H2O will have a mass of 48 * 18 = 864 g.

The balanced chemical equation also shows that for every 2 moles of C3H8O that react, 6 moles of CO2 are produced. Therefore, 6 moles of C3H8O will produce 6 * 3 = 18 moles of CO2.

The molar mass of CO2 is 44 g/mol. Therefore, 18 moles of CO2 will have a mass of 18 * 44 = 792 g.

Therefore, the combustion of 6 moles of C3H8O will produce 864 g of H2O and 792 g of CO2.