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18 January, 05:24

Consider the reaction between 50.0 ml liquid methanol, ch3oh (density 0.850 g/ml), and 22.8 l o2 at 27c and a pressure of 2.00 atm. the products of the reaction are co2 (g) and h2o (g). calculate the number of moles of h2o formed if the reaction goes to completion.

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  1. 18 January, 07:24
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    The reaction balanced equation is:

    2CH3OH + 3O2 → 2CO2 + 4 H2O

    the no. of moles of CH3OH = Mass of CH3OH / molar mass of CH3OH

    when the mass of CH3OH = volume * density of CH3OH

    = 50 * 0.850 = 42.5 g

    ∴no of moles of CH3OH = 42.5 g / 32 g/mol = 1.328 moles

    after that to get the no. of moles of the gas O2 we have to decrease the T from 27 °C to zero and the pressure from 2 atm to 1 atm to get the corrected volume to STP.

    So by substitution in this formula:

    no. of moles of O2 = difference T in Kelvin * volume * change in pressure/molar volume

    when we have difference T in kelvin to get V correction = 273K / (27°C+273K) = 0.91 K

    and Volume in the start = 22.8 L

    the change in pressure = 2atm/1atm = 2 atm

    and the molar volume = 22.4 L (as according to STP 1 mole of any gas occupies 22.4 L)

    So by substitution:

    no. ofmoles of O2 = (0.91 * 22.8 * 2) / 22.4 = 1.832 moles

    and according to the balanced equation:

    ∴ the no. of moles of H2O = no. ofmoles of O2 * (4 mol H2O / 3 mol O2)

    = 1.832 * (4/3) = 2.44 moles
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