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15 May, 04:55

Oxygen gas, generated by the reaction 2KClO3 (s) - >2KCl (s) + 3O2 (g) is collected over water at 27°C in a 1.55 L vessel at a total pressure of 1.00 ATM. (the vapor pressure of H2O at 27°C is 26.0 torr.) how many moles of KClO3 were consumed in the reaction?

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  1. 15 May, 05:04
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    Use Dalton's law and the vapor pressure of water at 23.0 o C to correct the pressure to units of atmoshperes.

    PT = Poxygen + Pwater

    At 23.0 o C the vapor pressure of water is 21.1 mmHg. (This can be found on a vapor pressure table.)

    762 mmHg = Poxygen + 21.1 mmHg

    Poxygen = 762 mmHg - 21.1 mmHg

    Poxygen = 741 mmHg

    Convert the corrected pressure to atmospheres.

    (741 mmHg) (1 atm / 760 mmHg) = 0.975 atm

    Use the ideal gas law to find out how many moles of gas were produced:

    PV = nRT (remember to put volume in liters and temperature in Kelvin)

    (0.975 atm) (.193 L) = n (.0821 L atm / mol K) (298 K)

    n = (0.975 atm) (.193 L) / (.0821 L atm / mol K) (298 K)

    n = 7.69 X 10-4 mol

    Use the number of moles and the molecular weight of oxygen to find out how many grams of oxygen were collected.

    (7.69 X 10-4 mol) (32.0 g / 1 mol) = 2.46 X 10-2 g
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