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28 May, 17:14

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) ?

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  1. 28 May, 17:28
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    For the complete combustion of 3.0 moles CH4 we need 6.0 moles O2

    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
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