Question

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.

Answer 1

Answer:

Explanation:

The pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual gases:

Σ$P_g_a_s$ $= P_1+P_2+P_3+...+P_n$

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:

$P_g_a_s=1 \ atm = 760 \ torr= P_N_2+P_O_2+P_C_O_2\\760 \ torr = 582.008 \ torr + P_O_2 \ + 0.285 \ torr$

Solve for Po2:

$P_o_2=(760-582.008-0.285) \ torr = 177.707 \ torr$

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

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