in a sample containing a mixture of only these gases at exactly one atmosphere pressure, the partial pressures of carbon dioxide and nitrogen are given as Pco2= .285 torr and PN2= 582.008 torr. What is the partial pressure of oxygen?
Answer in units of torr.

The prompt is trying to confuse you, but it actually tells us the pressure of the mixture to be 1 atm, but this can be converted to torr. Furthermore, we are informed only three gases are in the mixture: diatomic nitrogen, diatomic oxygen, and carbon dioxide:

[tex]P_g_a_s=1 \ atm = 760 \ torr= P_N_2+P_O_2+P_C_O_2\\760 \ torr = 582.008 \ torr + P_O_2 \ + 0.285 \ torr[/tex]

Solve for Po2:

[tex]P_o_2=(760-582.008-0.285) \ torr = 177.707 \ torr[/tex]

Thus, the partial pressure of diatomic oxygen is 177.707 torr.

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in a sample containing a mixture of only these gases at exactly one atmosphere pressure, the partial pressures of carbon dioxide and nitrogen are given as Pco2= .285 torr and PN2= 582.008 torr. What is the partial pressure of oxygen? Answer in units of torr.

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in a sample containing a mixture of only these gases at exactly one atmosphere pressure, the partial pressures of carbon dioxide and nitrogen are given as Pco2= .285 torr and PN2= 582.008 torr. What is the partial pressure of oxygen?
Answer in units of torr.