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Concept explainers
Interpretation:
For a given sample of water in closed container the molecules of water present under given volume should be determined.
Concept Introduction:
Ideal gas Equation:
Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation.
Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties. At lower temperature and at high pressures the gas tends to deviate and behave like real gases.
Boyle’s Law:
At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume.
Charles’s Law:
At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature.
Avogadro’s Hypothesis:
Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it.
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Chapter 10 Solutions
Chemistry & Chemical Reactivity
- If 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_forwardYou have two pressure-proof steel cylinders of equal volume, one containing 1.0 kg of CO and the other containing 1.0 kg of acetylene, C2H2. (a) In which cylinder is the pressure greater at 25 C? (b) Which cylinder contains the greater number of molecules?arrow_forwardAnswer the following questions: (a) If XX behaved as an ideal gas, what would its graph of Z vs. P look like? (b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified? (c) What is the effect of the volume of gas molecules on Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (d) What is the effect of intermolecular attractions on the value of Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (e) In general, under what temperature conditions would you expect Z to have the largest deviations from the Z for an ideal gas?arrow_forward
- A sample of an ideal gas at 1.00 atm and a volume of 1.09 I was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 80.0 atm, what was the volume of the sample? Assume that the temperature was held constant.arrow_forwardA typical barometric pressure in Redding, California, is about 752.03 mmHg. Calculate this pressure in atm.arrow_forwardEach sketch below shows a flask with some gas and a pool of mercury in it. The gas is at a pressure of 1 atm. A J-shaped tube is connected to the bottom of the flask, and the mercury can freely flow in or out of this tube. (You can assume that there is so much more mercury in the pool than can fit into the tube that even if the J-tube is completely filled, the level of mercury in the pool won't change.) Notice also that in the left sketch the J-tube is open at its other end, so that air from the atmosphere can freely flow. On the other hand, in the right sketch the J-tube is closed at its other end, and you should assume there is no gas between the mercury and the closed end of the tube. To answer this question, you must decide what the mercury level will be when the mercury finally stops flowing in or out of the tube. By moving the sliders back and forth, you'll see different levels of mercury in the J-tube. Select the final correct level for each sketch. 1 1 2 I Don't Know open tube…arrow_forward
- Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains C2H4 flask B contains O 3 , and flask C contains F 2 . Which flask contains the largest number of molecules?arrow_forwardChemistry An empty flask weighs 129.361 g. After vaporization of a sample of volatile liquid at a temperature of 99.7 °C, the flask was sealed, cooled to room temperature, and found to have a mass of 129.657 g. The atmospheric pressure was 759.1 mm Hg. The flask was rinsed and completely filled with water at 23.4 °C. The mass of the water-filled flask was determined to be 377.398 g. What is the temperature of the gas that fills the flask in Kelvin? (Enter your answer as a number without units.) An empty flask weighs 128.950 g. After vaporization of a sample of volatile liquid at a temperature of 99.4 °C. the flask was sealed, cooled to room temperature, and found to have a mass of 129.368 g. The atmospheric pressure was 759.5 mm Hg. The flask was rinsed and cormpletely filled with water at 21.3 °C. The mass of the water-filled flask was determined to be 377.557 g. What is the molar mass (in g/mol) of the volatile liquid? (Enter your answer as a number without units.)arrow_forward10. A gaseous mixture that contains 0.0500 mol each of N₂, H₂, and He is kept in a cylinder with a volume of 10.00 L and exerts a total pressure of 746 mmHg. (a) What is the temperature (in °C) at which the gas exists? (b) What is the partial pressure (in atm) of He in the mixture? 11. A gaseous mixture that contains 200 mg each of N₂, H₂, and He is kept in a cylinder with a volume of 10.00 L and exerts a total pressure of 746 mmHg. (a) What is the temperature (in °C) at which the gas exists? (b) Which gas exerts the greatest partial pressure?arrow_forward
- 3a. Write down the two versions of the Ideal Gas Law and define each term and its units. 3b. How much volume (in liters) is occupied by 1.5 moles of an ideal gas at STP? (hint: first define STP).3c. What is the new volume (in liters) if the temperature is increased to room temperature (295 K) keeping pressure constant?arrow_forwardEach sketch below shows a flask with some gas and a pool of mercury in it. The gas is at a pressure of 0.5 atm. A J-shaped tube is connected to the bottom of the flask, and the mercury can freely flow in or out of this tube. (You can assume that there is so much more mercury in the pool than can fit into the tube that even if the J-tube is completely filled, the level of mercury in the pool won't change.) Notice also that in the left sketch the J-tube is open at its other end, so that air from the atmosphere can freely flow. On the other hand, in the right sketch the J-tube is closed at its other end, and you should assume there is no gas between the mercury and the closed end of the tube. To answer this question, you must decide what the mercury level will be when the mercury finally stops flowing in or out of the tube. By moving the sliders back and forth, you'll see different levels of mercury in the J-tube. Select the final correct level for each sketch. A open tube closed tube -…arrow_forward73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)arrow_forward
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