# Problem: Consider the following unbalanced chemical equation for the combustion of pentane (C5H12):C5H12 (l) + O2 (g) → CO2 (g) + H2O (l)If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?

###### FREE Expert Solution

We're being asked to calculate the mass of water that can be produced from 20.4 g of pentane. We're given the following unbalanced reaction:

C5H12 (l) + O2 (g) → CO2 (g) + H2O (l)

We have to balance the reaction first:

Reaction:

 ___ C5H12(l) + ___ O2(g) → ___ CO2(g) + ___ H2O(l) C         5 C         1 H         12 H         2 O         2 O         3

Balance C: We have 5 C on the reactant side and 1 C on the product side – add a coefficient of 5 to CO2:

 ___ C5H12(l) + ___ O2(g) → 5 CO2(g) + ___ H2O(l) C         5 C         5 H         12 H         2 O         2 O         11

Balance H: We have 12 H on the reactant side and 2 H on the product side – add a coefficient of 6 to H2O:

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###### Problem Details

Consider the following unbalanced chemical equation for the combustion of pentane (C5H12):

C5H12 (l) + O2 (g) → CO2 (g) + H2O (l)

If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?