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Given the reaction: CH4(g) + 2 O2 (g)  CO2(g) + 2H2O(g) How many moles of oxygen are needed for the complete combustion of 3.0 moles of CH4(g)?

2 Answers

4 votes

Answer:

6 moles are needed

Step-by-step explanation:

User Jiaxiang
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2 votes

Answer:

For the complete combustion of 3.0 moles CH4 we need 6.0 moles O2

Step-by-step explanation:

Step 1: Data given

Number of moles of CH4 = 3.0 moles

Step 2: The balanced equation

CH4(g) + 2 O2 (g) → CO2(g) + 2H2O(g)

Step 3: Calculate moles of O2

For 1 mol CH4 we need 2 moles of O2 to produce 1 mol of CO2 and 2 moles of H2O

For 3.0 moles CH4 we need 2* 3.0 = 6.0 moles of O2

To produce 3.0 moles of CO2 and 6.0 moles H2O

For the complete combustion of 3.0 moles CH4 we need 6.0 moles O2

User Paul Razvan Berg
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