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A mixture of 2.00 moles of H2, 3.00 moles of NH3, 4.00 of CO2 and 5.00 moles of N2...

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bluebutterfly... | Student | eNoter

Posted May 9, 2013 at 8:43 PM via web

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A mixture of 2.00 moles of H2, 3.00 moles of NH3, 4.00 of CO2 and 5.00 moles of N2 exerts a total pressure of 800.0 torr. What is the partial pressure of each gas? Please help I don't understand chemistry.

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jerichorayel | College Teacher | (Level 1) Senior Educator

Posted May 10, 2013 at 12:56 AM (Answer #1)

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The partial pressure of a certain gas in a container of other gasses can be expressed as:

`P_a = (f_a)*P_(t otal)`

Where:

`f_a` is the mole fraction of gas a

`Mol e f r a c t ion = (n_a)/(n_(t otal))`

`P_(t otal)` = total pressure exerted by the gasses.

 

`T otal mol es = n_(t otal) = n_(H_2) + n_(NH_3) + n_(CO_2) + n_(N_2)`

`T otal mol es = n_(t otal) = 2.00 + 3.00 + 4.00 + 5.00`

`T otal mol es = n_(t otal) = 14.0 mol es`

 

Total pressure = 800 torr

Partial pressures: (answers)

`p_(H_2) = 2.00/14.00 * 800 = 114 t o rr`

`p_(NH_3) = 3.00/14.00 * 800 = 171 t o rr`

`p_(CO_2) = 4.00/14.00 * 800 = 229 t o rr`

`p_(N_2) = 5.00/14.00 * 800 = 286 t o rr`

Sources:

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