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Mole to mole problems?

Consider the equation: 2 CH3OH + 3O2 —> 2 CO2 + 4 H2O If 3.5 moles of methanol are burned in an abundant supply of oxygen and one mole) How much oxygen is used? b) How many moles of H20 are produced? I understand how find the molar mass and molar and such, but these are the Mole and Mole to Mass to Mole problems that confuse me: s. Any ideas?

You can see in the equation for 2 moles of CH3OH you need 3 moles of O2. Or you can say it is a ratio of 2:3 or 1 for each mole of CH3OH using 1.5 moles of O2. Therefore, your answer to a. is 3.5 * 1.5 = 5.25 moles of O2 are used. For b. you can see in equation that for 2 moles of CH3OH used 4 moles of H2O is produced. Or you can see twice as much H2O is produced from CH3OH is used. So you're responding to b. is 3.5 * 2 = 7 moles of H2O are produced.

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