Concept explainers
Interpretation:
Partial pressure of each gas in a flask that contains
Concept Introduction:
The net pressure of a mixture of gases is equal to the sum of the partial pressures of its constituent gases. This is known as Dalton’s law of partial pressure.
The total pressure for a mixture of two gases A and B is calculated as follows:
In terms of mole fraction the partial pressure is calculated as follows:
Here,
Answer to Problem 6.86QE
Partial pressure exerted by each gas in a flask that contains
Explanation of Solution
The formula to convert mass in gram to moles is as follows:
Substitute
Substitute
Substitute
The formula to calculate mole fraction is as follows:
Here,
Substitute
In terms of mole fraction the partial pressure is calculated as follows:
Here,
Substitute 0.974 for
The formula to calculate mole fraction is as follows:
Here,
Substitute
In terms of mole fraction the partial pressure is calculated as follows:
Here,
Substitute 0.002136 for
The formula to calculate mole fraction is as follows:
Here,
Substitute
In terms of mole fraction the partial pressure is calculated as follows:
Here,
Substitute 0.02349 for
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Chapter 6 Solutions
Chemistry: Principles and Practice
- A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?arrow_forwardHydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.arrow_forwardIf equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.arrow_forward
- The following figure shows three 1.00-L bulbs connected by valves. Each bulb contains argon gas with amounts proportional to the number of circles pictorially represented in the chamber. All three bulbs are maintained at the same temperature. Unless stated otherwise, assume that the valves connecting the bulbs are closed and seal the gases in their respective chambers. Assume also that the volume between each bulb is negligible. (a) Which bulb has the highest pressure? (b) If the pressure in bulb A is 0.500 atm, what is the pressure in bulb C? (c) If the pressure in bulb A is 0.500 atm, what is the total pressure? (d) If the pressure in bulb A is 0.500 arm, and the valve between bulbs A and B is opened, redraw the figure shown above to accurately represent the gas atoms in all three bulbs. What is P A+P B+P C? Compare your answer in part (d) to that in part (c). (e) Follow the instructions of part (d) but now open only the valve between bulbs B and C.arrow_forwardA mixture at 33 °C contains H2at 325 torr. N;at 475 tore and O2at 650. torr. What is the total pressure of the gases in the system? Which gas contains the greatest number of moles?arrow_forward
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