# Problem: How many moles of O 2 (molar mass = 32.00 g/mol) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO 2 and H2O? (molar mass (CH 4) = 16.04 g/mol)a) 11.6b) 2.32c) 4.64d) 52.0e) 104

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88% (352 ratings)
###### FREE Expert Solution

We will calculate the moles of O2 needed to react with 52.0 L of CH4 using mole to mole comparison.

Let’s first write a balanced reaction equation. We know that the reaction is a combustion reaction since CH4 is made of carbon and hydrogen and is combusted to form carbon dioxide and water as products.

Reaction Equation: CH4 + O2 → CO2 + H2O

C is balanced

Balance H:               CH4 + O2 → CO2 + 2 H2O

Balance O:               CH4 + 2 O2 → CO2 + 2 H2O

Reactant            Product

C 1                      C  1
H  4                     H  2 4
O  2 4                  O  3 4

Balanced reaction Equation: CH4 + 2 O2 → CO2 + 2 H2O

88% (352 ratings) ###### Problem Details

How many moles of O 2 (molar mass = 32.00 g/mol) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO 2 and H2O? (molar mass (CH 4) = 16.04 g/mol)

a) 11.6

b) 2.32

c) 4.64

d) 52.0

e) 104

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