A mixture of gases contains 810 g of n2 190 g of h2 and 350
A mixture of gases contains 8.10 g of N2, 1.90 g of H2, and 3.50 g of NH3. If the total pressure of the mixture is 2.60 atm, what is the partial pressure of each component?
PN2 =_______ atm
PH2 =_______ atm
PNH3 =_______ atm
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Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.)
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For a person with a hematocrit of 0.45, the arterial blood has an oxygen partial pressure of 100 mmHg. (1) What is the concentration of dissolved oxygen in the blood (2) How does your answer in (1) compare to the oxygen requirement
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A mixture containing 2.01 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture.
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