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12 May, 09:08

let 4 moles of methanol (liquid) combust in 3 moles of gaseous oxygen to form gaseous carbon dioxide and water vapor. Suppose this occurs in a chamber of fixed volume and fixed temperature. If the original pressure is 1.0 atm, what is the final pressure in the chamber. Express your answer in atm. Enter a numerical value, do not enter units. Assume liquids take up negligible volume.

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  1. 12 May, 11:58
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    The final pressure is 2.0 atm

    Explanation:

    Step 1: Data given

    Number of moles methanol = 4 mol

    Number of moles oxygen = 3 mol

    original pressure is 1.0 atm

    Step 2: The balanced equation

    2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l)

    Step 3: Calculate final pressure

    For 2 moles of methanol consumed, we need 3 moles O2 to produce 2 moles CO2 and 4 moles H2O

    We started with 3 moles of O2 gas.

    Since methanol is not a gas, it doesn't count for the pressure.

    V and T are fixed

    This means the final pressure can be given by:

    P2/P1 = n2/n1

    with n2 = number moles of products

    with n1 = number of moles of reactants

    P2 = (6.0 mol*1.0 atm) / (3.0 mol)

    P2 = Final pressure = 2.0 atm
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