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A mixture is placed in a spherical container. It contains oxygen at , carbon dioxide at , and nitrogen at . What is the total pressure of the mixture?

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General Chemistry 1

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Solve problems relating to Dalton's Law of Partial Pressures

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If the total pressure of a mixture is

, which consists of carbon dioxide at

and nitrogen. Determine the partial pressure of

A mixture of gas in a container is at . If Gas A has of pressure, Gas B has of pressure, Gas C has of pressure, what is the partial pressure of Gas D in ?

HELP!!! I want to know the step by step process to solve these problems. Italicized and bolded are the answers.

1.) A tank contains 17.00 moles total of carbon dioxide, nitrogen, and oxygen. Calculate the moles of carbon dioxide, if the percent of nitrogen is 44 % and oxygen is 31%. (Hint, convert percent into mole fraction.) 4.2 (4.25) mol Carbon dioxide

2.) A quantity of nitrogen gas originally at 4.60 atm in a 1.20 L container at 23.9 ÂºC is transferred to a 10.0 L container. A quantity of oxygen originally at 3.50 atm and 23.9 ÂºC in a 4.00 L container is transferred to the same 10.0 L container with the ni trogen. Calculate the total pressure of the two gases in the 10.0 L container at 19.7 ÂºC. 1.93 atm

3.) A 50.00 liter tank at - 15.00 Â°C contains 14.00 grams of helium gas and 10.00 grams of nitrogen gas.

a. Determine the total pressure in the tank. P_T = 1.632 atm

b. Determine the partial pressure of each gas. P _He = 1.481 atm PN2 = 0.1512 atm

c. Determine the volume at STP. 86.33 L

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A mixture is placed in a spherical container. It contains oxygen at , carbon dioxide at , and nitrogen at . What is the total pressure of the mixture?

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