C5H12 (g) + O2 (g) —> CO2 (g) + H209 (g) ( Needs Balance )
Please explain how to find the answer also.Thanks!
2 Answers

Balanced equation: C5H12(g) + 8 O2(g) > 5 CO2(g) + 6 H2O
Given mol C5H12 x mole ratio(mol H2O/mol C5H12) = mol H2O
The mole ratio is obtained from the coefficients of the BALANCED equation: 6 mol H2O : 1 mol C5H12
0.100 mol C5H12 x (6 mol H2O/1 mol C5H12) = 0.6 mol H2O
Sig figs… 0.600 mol H2O

Ok, first step is to set up a balanced equation with which you can use stoicheometry to go from pentane to water.
in this case the balanced equation looks like:
1(C5H12)+8(O2)–>5(CO2)+6(H20)
What this tells you is that for every one mole of pentane burned 6 moles of water is released, making the stoicheometric factor (6molH20)/(1molC5H12)
you can then multiply .100molC5H12 by (6molH20)/(1molC5H12) , the “molC5H12” cancels out and you are left with .600 moles of water
——>.600 moles of water<——