Explanation:
Automobile tires are typically inflated to about 30 pounds of pressure per square inch. What is the typical air pressure of a tire in kPa?
206 KPa
When temperature-volume measurements are made on 1.0 mol of gas at 1.0 atm, a plot V versus T results in a
Straight line
3. A syringe initially holds a sample of gas with a volume of 285 mL at 355 K and 1.88 atm. To what temperature must the gas in the syringe be heated/cooled in order to have a volume of 435 mL at 2.50 atm?
720.0 K
At the same temperature and the same volume, a 20.0 grams sample of each of He, H2 , O2 or Cl2 were placed in three different flasks. Which gas will have the lowest pressure? Which will have the highest pressure?
(Cl2 will have the lowest pressure). (H2 will have the highest pressure).
The highest pressure ever produced in a laboratory setting was about 2.0 x 106 atm. If we have a 1.0 x 10-5 liter sample of a gas at that pressure, then release the pressure until it is equal to 0.275 atm, what would the new volume of that gas be?
(V2=73 L)
6. A soda bottle is flexible enough that the volume of the bottle can change even without opening it. If you have an empty soda bottle (volume of 2 L) at room temperature (25 0C), what will the new volume be if you put it in your freezer (-4 0C)?
2L
A balloon contains 0.128 mol of gas and has a volume of 2.76L. if an additional 0.073 mol of gas is added to the balloon ( at the same temperature and pressure ), what will its final volume be?
(V2=4.33 L)
An "empty" aerosol can at 25 °C still contains gas at 1.00 atmosphere pressure. If an "empty" can is thrown into a 475 °C fire, what is the final pressure in the heated can?
(P2=2.51 atm)
Under what condition is a sample of gas most likely to behave ideally?
(At STP, where the temperature is 273 K and the pressure is 1.00 atm).
Calculate the pressure exerted by 0.39 mol of methane (CH4) in a container of volume 3.5L at 390 C?
(P= 2.9 atm).
How many molecules of N2 are in a 500.0 mL container at 780 mm Hg and 135 °C?
(9.23 x 1021 molecules of N2)
A 75.0 L steel tank at 20.0 °C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank?
(113 g C2H2).
A steel bottle contains argon gas at STP. What is the final pressure if the temperature is changed to 115 °C?
(P2= 1.42 atm).
A 0.286-g sample of gas occupies 125 mL at 60. cm of Hg and 25 °C. What is the molar mass of the gas?
(70.9 g/mol).
What is the density of fluorine gas at STP?
1.70 g/L
What is volume of 12 gram of He at STP?
(V=67 L He).
What is density of 12 gram of He at STP?
(0.179 g/L).
8. What is volume of 12 mole of He at STP?
(V=270 L He).
One mole of which gas has the greatest density at STP?
A) Ar
B) N2
C) CO
D) All three gases have the same density.
Ar (has the highest Molar Mass.)
Which of the following would have a density of 1.21 g/L at 7.0 °C and 0.987 atm?
N2
The followings are assumed in identical flasks at the same temperature and the same pressure (STP). When a 20.0 grams sample of each of He, H2 , O2 or Cl2 are placed in three different flasks, Which one will have highest density?
(Cl2; highest molar mass=highest Density).
What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K?
(86.7 g NO2).
Which one of the followings He, H2 , O2 or Cl2 has the greatest density at STP?
Cl2
930g sample of an unknown compound occupies 490 mL at 298 K and 2.44atm. What is the molar mass of the unknown compound? Hint: calculate n, MM= (Gram/mol) or (g/n)
(MM=19000 g/mol).
