Gaseous and liquid states Questions and Answers

The volume of gas is increased from 150.0 ml to 350.0 mL by heating it. If the original temperature was 25.0°C, what will be the final temperature of the gas (in °C), assume that the pressure is constant. 146°C 10.7°C 58.3°C 422°C 695°C

A sample of sulfur hexafluoride gas occupies 9.39 L at 299°C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 4.43 L? Report your answer to the proper number of significant figures.

Three 8-L flasks, fixed with pressure gauges and small valves, each contain 1 g of gas at 284 K. Flask A contains CH4, flask B contains H₂, and flask C contains He. Rank the flask contents in terms of: (a) pressure. A>B>C A> C> B B> C>A B>A>C C> B>A C>A>B A=B=C (b) average molecular kinetic energy. A>B>C A> C> B B> C>A B>A>C C>B>A C>A>B A=B=C

How do twentieth-century composers handle rhythm? Rhythms are often mixed with polyrhythm used commonly. Rhythms are generally from African rather than from European music. Rhythms are fairly common with consistent beats in each measure. Rhythms are often static rather than dynamic.

A helium-filled balloon of the type used in long-distance flying contains 420,000 ft (1.2 x 107 L) of helium. Suppose you fill the balloon with helium on the ground, where the pressure is 739 mm Hg and the temperature is 17.8 °C. When the balloon ascends to a height of 2 miles, where the pressure is only 600. mm Hg and the temperature is -33 °C, what volume is occupied by the helium gas? Assume the pressure inside the balloon matches the external pressure.

A flask is first evacuated so that it contains no gas at all. Then, 2.3 g of CO2 is introduced into the flask. On warming it to 32.0 °C, the gas exerts a pressure of 323 mm Hg. What is the volume of the flask?

Two containers, at identical temperature and pressure, hold gaseous chloriney The volume of container 1 is 1.03 L, and it contains 6.1 mol of the gas. container 2 is 2.25 L. How many moles of the gas are in container 2?

For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of -196. °C. Suppose the temperature of a sample of nitrogen gas is raised from 90.0 °C to 126.0 °C, and at the same time the pressure is decreased by 15.0%. Does the volume of the sample increase, decrease, or stay the same? If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent.

A reaction at 14.0 °C evolves 454. mmol of carbon monoxide gas. Calculate the volume of carbon monoxide gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits.

One liter of a gas is in a sealed chamber containing a moveable piston. If the piston is moved so that the volume of the gas is compressed to a volume of one-half liter, what will happen to the pressure on the gas? (Assume the temperature is constant and no gas particles are lost.) The pressure will remain the same. The pressure will be twice the original value. The pressure will be half of the original value. It would be impossible to move the piston since gases are not compressible.

A reaction between liquid reactants takes place at 11.0 °C in a sealed, evacuated vessel with a measured volume of 5.0 L. Measurements show that the reaction produced 39. g of dinitrogen difluoride gas. Calculate the pressure of dinitrogen difluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.

For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of -33. °C. Suppose the temperature of a sample of ammonia gas is raised from 10.0 °C to 10.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.59 kPa and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits.

A sample of an unknown compound is vaporized at 200. °C. The gas produced has a volume of 2110. mL at a pressure of 1.00 atm, and it weighs 1.85 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

A sample of an unknown compound is vaporized at 140. °C. The gas produced has a volume of 2130. ml. at a pressure of 1.00 atm, and it weighs 8.63 8. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

What is the internal energy of 7.00 mol of N₂ gas at 40°C? To solve this problem, use the equation: Udiatomic gas=5/2nRT Remember that R= 8.31 J/(mol-K) and K = °C + 273. A. 45,500 J B. 11,600 J CC. 5820 J D. 18,200 J

A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 99.5 kPa. The piston is now pulled up, expanding the gas, until the gas has a final volume of 23.0 L. Calculate the final pressure of the gas. Round your answer to 3 significant digits.

An arctic weather balloon is filled with 16.9 L of helium gas inside a prep shed. The temperature inside the shed is 13. °C. The balloon is then taken outside, where the temperature is -20. °C. Calculate the new volume of the balloon. You may assume the pressure on the balloon stays constant at exactly 1 atm. Round your answer to 3 significant digits.

The typical pressure of carbon dioxide in an unopened soda can is 2.63 x 10³ mmHg. Calculate the typical pressure in atm and torr. Round each of your answers to 3 significant digits. atm torr

A reaction between liquid reactants takes place at -6.0 °C in a sealed, evacuated vessel with a measured volume of 35.0 L. Measurements show that the reaction produced 25. g of sulfur hexafluoride gas. Calculate the pressure of sulfur hexafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits. pressure: atm

Boron trifluoride gas is collected at -18.0 °C in an evacuated flask with a measured volume of 45.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.460 atm. Calculate the mass and number of moles of boron trifluoride gas that were collected. Round your answer to 3 significant digits.

An arctic weather balloon is filled with 36.9 L of helium gas inside a prep shed. The temperature inside the shed is 6. °C. The balloon is then taken outside, where the temperature is -34. °C. Calculate the new volume of the balloon. You may assume the pressure on the balloon stays constant at exactly I atm. Round your answer to 3 significant digits.

The atmospheric pressure on top of Mt. Everest (elevation 29,028 ft) is 0.329 atm. Calculate the atmospheric pressure in mmHg and torr, Round each of your answers to 3 significant digits. mm Hg torr

Which of the following represents the law of heat exchange? Heat lost #Heat gained Heat lost Heat gained Heat lost > Heat gained Heat lost = Heat gained

An arctic weather balloon is filled with 24.6 L of helium gas inside a prep shed. The temperature inside the shed is 11. °C. The balloon is then taken outside, where the temperature is - 12. °C. Calculate the new volume of the balloon. You may assume the pressure on the balloon stays constant at exactly 1 atm. Round your answer to 3 significant digits.

16) Standard temperature and pressure (STP), in the context of gases, refers to A) 298.15 K and 1 atm B) 273.15 K and 1 atm C) 298.15 K and 1 torr D) 273.15 K and 1 pascal E) 273.15 K and 1 torr

18) An ideal gas differs from a real gas in that the molecules of an ideal gas A) have no attraction for one another B) have appreciable molecular volumes C) have a molecular weight of zero D) have no kinetic energy E) have an average molecular mass

In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is ___ if the partial pressures of He and Ne are 1.50 and 2.00 atm, respectively. A) 0.48 B) 0.58 C) 0.68 D) 0.78 E) 0.88

A sample of carbon dioxide gas at a pressure of 1.07 atm and a temperature of 106°C, occupies a volume of 686 ml. If the gas is heated at constant pressure until its volume is 013 mL, the temperature of the gas sample will be

On a relative basis, the weaker the intermolecular forces in a substance are, a. the more it deviates from the ideal gas law. b. the higher is its boiling point. c. the larger is its molar heat capacity as a liquid. d. the larger is its heat of vaporization. e. the greater is its vapor pressure at a particular temperature.

A sample of hydrogen gas occupies a volume of 9.86 L at 59.0°C and 0.420 atm. If it is desired to increase the volume of the gas sample to 12.5 L, while increasing its pressure to 0.574 atm, the temperature of the gas sample at the new volume and pressure must be __ C

A sample of xenon gas at a pressure of 1.20 atm and a temperature of 29.4°C, occupies a volume of 10.4 L. If the gas is allowed to expand at constant temperature to a volume of 18.5 L, the pressure of the gas sample will be atm

A sample of argon gas at a pressure of 0.894 atm and a temperature of 199°C, occupies a volume of 853 mL. If the gas is heated at constant pressure until its volume is 998 mL, the temperature of the gas sample will be °C.

A sample of oxygen gas occupies a volume of 6.49 L at 50.0°C and 366 torr. If the volume of the gas sample is decreased to 4.68 L, while its temperature is decreased to -9.0°C, the resulting gas pressure will be torr.

A sample of hydrogen gas occupies a volume of 9.13 L at 61.0°C and 333 torr. If the volume of the gas sample is increased to 10.5 L, while its temperature is decreased to 10.0°C, the resulting gas pressure will be __torr.

4. Finding the pressure at 18 nm³. a.. Using the power equation, find the pressure at 18 nm³.

The atmosphere of the planet Venus is mostly carbon dioxide gas. At the surface of the planet, the temperature is 801°C with a pressure of 7.50 x 10 kPa. If these are STP conditions on Venus, what would be the molar volume of carbon dioxide gas? (Hint: use STP conditions on Earth) [31]

A diatomic gas has a density at 4.14 g/L at a temperature of 3.0°C and pressure of kPa. Calculate the molar mass of the gas. Identify the gas (name), and provide the chemical formula for it. [4T]

Scuba divers use tanks of compressed air to help them breathe. Gases can be compressed because (select all that apply) A. the volume of the gas particles is small compared to the overall volume of the gas B. the distance between gas particles is less than the distance between particles of a liquid or solid C. there is empty space between the particles of a gas D. gas particles are moving faster than the particles of a liquid or solid

2. Which of the following shows the correct way to rearrange this equation to solve for the unknown? A. PN₂ = Pair - (Po₂ + Pco₂+ Pothers) B. Pothers = Pair + PCO₂ + PO₂ + PN₂ C. PN₂ = Pair - PO₂ + Pothers + Pco₂ D. Pair = PN₂ + Po₂ + Pco₂ + Pothers

Nitrogen and oxygen combine to form nitrogen dioxide according to the balanced equation below. How many grams of nitrogen dioxide can be produced when 34.5 g of nitrogen reacts with 52.6 g of oxygen? N₂+2 0₂2 NO₂ moles N₂ moles O₂ limiting reactant ("nitrogen" or "oxygen") moles NO₂ produced grams NO₂ produced

The pressure in an automobile tire filled with air is 245.0 kPa. Air is a mixture of gases containing nitrogen, oxygen, carbon dioxide, and other gases. Find PN₂ if Po₂ = 51.3 kPa, Pco₂ = 0.10 kPa, and Pothers = 2.3 kPa. What is the unknown in this problem? A. Ptotal B. PcO₂ C. PN₂ D. PO₂ E. Pothers

Sodium carbonate and hydrochloric acid react according to the following equation: Na₂CO3 + 2 HCI → CO₂ + H₂O + 2 NaCl How many liters of CO₂ at STP can be produced from 13.5 g of sodium carbonate and an excess of HCI? moles Na₂CO3 ___ moles of CO₂ ___ volume of CO2 ___

Compute the root-mean-square speed of N₂ molecules in a sample of nitrogen gas at a temperature of 201°C. 20.52 ms

As 1 g of the radioactive element radium decays over 1 year, it produces 1.16 × 1018 alpha particles (helium nuclei). Each alpha particle becomes an atom of helium gas. What is the pressure in pascal of the helium gas produced if it occupies a volume of 125 mL at a temperature of 25 °C?

A gas mixture contains hydrogen, helium, neon, and argon. The total pressure of the mixture is 93.6 kPa. The partial pressures of helium, neon, and argon are 15.4 kPa, 25.7 kPa, and 35.6 kPa, respectively. What is the pressure exerted by hydrogen?

Which list ranks the gasses in the correct order from slowest to fastest rate of effusion? A. oxygen, chlorine, nitrogen, hydrogen B. hydrogen, oxygen, chlorine, nitrogen C. nitrogen, oxygen, hydrogen, chlorine D. chlorine, oxygen, nitrogen, hydrogen

A gas in a sealed container has a pressure of 272.1 kPa at a temperature of 20 °C. If the pressure in the container is changed to 188.6 kPa, what is the new temperature in °C ? Answer with no decimal place and the unit C (without the circle for degrees).

Gases, such as the air inside an inflated air bag, can be easily compressed because A. gas particles have mass B. gas particles are spaced far apart C. gases have high densities D. gas particles are constantly moving

A sample of nitrogen gas occupies a volume of 6.80 L at 50.0°C and 315 torr. If the volume of the gas sample is decreased to 4.92 L, while its temperature is decreased to -16.0°C, the resulting gas pressure will be __torr.

What volume of hydrogen gas is produced when 72.6 g of iron reacts completely according to the following reaction at 25 °C and 1 atm? iron (s) + hydrochloric acid(aq)-iron(II) chloride (aq) + hydrogen (g) liters hydrogen gas plning