Gas Laws/Solutions
If the pressure of the gas is 10 atm and the temperature is 298 K, calculate the volume of the balloon.
7.34 L
K2SO3 + 2 HCl 2 KCl + H2O +SO2 A 2.50 sample containing potassium sulfite and potassium iodide is analyzed by adding hydrochloric acid. The sulfur dioxide formed measured 320.0 mL when collected over water at 21C and a pressure of 804.1 mm Hg. What is the percent by mass of potassium sulfite in the original sample. (The vapor pressure of water at 21C is 18.7 mm Hg.)
86.7%
1.00 gram of propene gas occupies what volume at 147. C and 1.00 atm? A) 0.821 L B) 0.420 L C) 0.41L D) 1.64 L
A
A CH4 (molar mass 16 grams) effuses at 0.080 mole per minute at 289 K. At that temperature, a gas that effuses at approximately double that rate has what molar mass? A) 4 grams B) 8 grams C) 16 grams D) 32 grams
A
A balloon inflated with helium rises. Which of the following choices is the best explanation for this phenomenon? A) The density of helium gas is less than that of the surrounding air. B) The inside of the balloon is warmer than the outside. C) Outside pressure forces the balloon upwards. D) The cooler air surrounding the ballon pushes against the side of the balloon.
A
A gaseous mixture contains 4.5 moles hydrogen, 2.0 moles nitrogen, and 3.5 moles neon. This system exerts a total pressure of 0.80 atmosphere. What is the partial pressure of the hydrogen? A) 0.36 atm B) 0.42 atm C) 0.57 atm D) 0.65 atm
A
A mixture of Cl2 gas and and O2 gas occupy a 1.000 L container at a pressure of 1200. torr. There are 3 times as many chlorine molecules as oxygen molecules. If the oxygen gas is removed from the mixture and placed inside an identical container (temperature is constant) what is the pressure inside the new container? A) 300. torr B) 600. torr C) 900. torr D) 1200. torr
A
A student wishes to prepare approximately 1.00 liter of a 0.200 m MgCl2 solution (formula mass 95.0 g). The proper procedure would be to weigh out A) 19.0 g of MgCl2 and 1.00 kg of water. B) 19.0 g of MgCl2 and 989. g of water. C) 19.0 g of MgCl2 and add water until final solution is approximately 1.00 liter. D) 95.0 g of MgCl2 and 1.00 kg of water.
A
Aqueous solutions of sugar (C6H12O6), NaCl, and HCl are all 10% solute by mass. Which represents them in order of increasing molarity? A) HCl < NaCl < C6H12O6 B) NaCl < C6H12O6 < HCl C) C6H12O6 < HCl < NaCl D) NaCl < HCl < C6H12O6
A
As temperature increases, solubility of which of the following decreases? A) NH3 B) NH4Cl C) NaNO3 D) KI
A
Base your answer to the following question on the elements below. (A) Chlorine (B) Silicon (C) Lead (D) Lithium Is a gas at room temperature A) A B) B C) C D)D
A
Base your answer to the following question on the following molecules. (A) H2 (B) O2 (C) Br2 (D) N2 Which molecule as a gas effuses the fastest? A) A B) B C) C D) D
A
C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g) A 0.03 mol sample of C3H8 is reacted with just enough O2 to use up both reactants in a 1 L flask at 300 K. The total pressure in the flask after the reaction is complete is closest to which of the following? ( Use R = 0.082 L atm mol-1 K-1) A) 5.0 B) 0.1 C) 0.25 D) 0.05
A
How many milliliters of 9.0-molar H2CO3 must be diluted to obtain 3.0 L of 6.0-molar H2CO3? A) 2000 mL B) 1175 mL C) 1050 mL D) 475 mL
A
Of the following organic compounds, which is LEAST soluble in water at 298 K? A) C6H6, benzene B) CH3Cl, chloromethane C) C2H5OH, ethanol D) C5H10O5, fructose
A
The pressure on a sample of gas is increased from 100 kPa to 130 kPa at constant temperature. Which of the following increases? I. The density of the gas II. The average distance between molecules III. The average speed of the molecules. A) I only B) III only C) I and II only D) I, II, and III
A
The total internal energy change for a gas is +2800. J. If it expanded from 2.000 liters to 4.000 liters against a pressure of 3.000 atm. What was the change in heat for the system? (1.00 L•atm = 101.0 J) A) -3406. J B) -2194. J C) +606. J D) +3406. J
A
The vapor pressure of acetic acid is 200. mmHg at 80.0oC. What is the vapor pressure at 80.0oC of a solution containing 0.250 mol of a non volatile substance dissolved in 6.50 mol of acetic acid? A) 193. mmHg B) 200. mmHg C) 207. mmHg D) 214. mmHg
A
Two containers for gases are at the same temperature and pressure. One contains 14.0 grams of nitrogen and the other 2.0 grams of helium. Which of the following is true? A) The volumes of the containers are the same. B) Both containers contain the same number of atoms. C) The average speed of the particles in both containers is the same. D) The density of the containers is the same.
A
What is the density of CO2 at 1.5 atm and 25 degrees Celcius? A) 2.7 g/L B) 5.4 g/L C) 10.8 g/L D) 32.2 g/L
A
What is the density of a gass that has a molar mass of 336 g/mol at STP? A) 15 g/L B) 150 g/L C) 168 g/L D) 336 g/L
A
What is the mole fraction of HF in a 10.% (by mass) solution? A) 0.090 B) 0.10 C) 0.90 D) 0.91
A
What is the total ion concentration in a 0.0500 M solution of Na3PO4? A) 0.200 M B) 0.150 M C) 0.100 M D) 0.050 M
A
When a sample of ethane gas in a closed container is cooled so that its absolute temperature halves, which of the following also halves? A) The average kinetic energy of the gas molecules B) The potential energy of the gas molecules C) The density of the gas D) The volume of the gas
A
Which method is best suited for separating a 500 mL sample of two miscible liquids whose boiling points differ by approximately 60°C? A) distillation B) evaporation C) fractional distillation D) paper chromatography
A
Which of the following gases is most like ideal? A) He B) SO2 C) H2O D) CO
A
Which of the following would increase the boiling point of a pure liquid in an open container? I. Dissolving 1 mol of any solid solute into the liquid II. Moving the liquid and container to a higher altitude III. Increasing the number of moles of liquid in the container A) I only B) II only C) III only D) I and III only
A
11. A rigid container filled with an ideal gas has its temperature raised from 283 K to 293 K. Which of the following increases? I. Average distance between the molecules II. Average speed of the molecules III. Density IV. Influence of particle-particle interaction A) I only B) II only C) I, II, and III only D) I, II, and IV only
B
A 1.00 L container at 460. K contains 3.23 moles of argon gas. What is the pressure of the gas? A) 1.24 × 104 atm B) 122. atm C) 244. atm D) 87.0 atm
B
A balloon filled with 0.01 mol of hydrogen gas is kept constant at 25 degrees Celcius. If the pressure is changed from 1 atm to 1.5 atm, what is the resulting volume of the balloon? A) 0.12 L B) 0.15 L C) 0.25 L D) 0.30 L
B
A certain first order reaction between two gases occurs at 389 K with a half-life of 24 hours. How much time is required to drop the pressure of one of the gases from 2.0 atm to 0.25 atm at 389 K? A) 8 hours B) 72 hours C) 192 hours D) 288 hours
B
A gas has a density of 0.600 g/L at a pressure of 0.1642 atm and a temperature of 127. C. What is the molar mass of the gas? A) 60.0 g/mol B) 120. g/mol C) 240. g/mol D) 360. g/mol
B
A gaseous mixture containing 6.5 moles of nitrogen, 2.0 moles of chlorine, and 1.5 moles of hydrogen exerts a total pressure of 0.70 atmosphere. What is the partial pressure of the chlorine? A) 0.07 atm B) 0.14 atm C) 0.26 atm D) 0.31 atm
B
A one mole solid sample of acetic acid (molecular wt.= 60 g/mol) is dissolved in 1.0 L of water to create a 1.0 molar solution. Which of the following would be the best procedure for determining the molality of the solution? A) Finding the volume of the solute B) Calculating the mass of the solvent C) Determining the specific heat of the solution D) Multiplying the molarity value by a factor of a thousand
B
A student wishes to prepare 3.00 liters of a 0.100 M HCl solution (formula mass 36.0 g). The proper procedure is to weigh out A) 10.8 g of HCl and 1.00 kg of water. B) 10.8 g of HCl and add water until the final solution has a volume of 3.00 liters C) 36.0 g of HCl and add water until the final solution has a volume of 3.00 liter. D) 10.8 g of HCl and add 3.00 liter of water.
B
An aqueous solution of concentrated HBr contains 48% HBr (MM = 80.9) by mass. The density of the solution is 1.50 g•mL-1 . What is the molarity of the HBr solution? A) 5.9 M B) 8.9 M C) 11.4 M D) 40.0 M
B
An ideal gas in a sealed container is heated from 290 K to 370 K at constant volume. Which of the following DO NOT change? I. The density of the gas II. The average distance between molecules III. The average speed of the molecules. A) I only B) I and II only C) I and III only D) I, II, and III
B
As a balloon floats higher, the surrounding air become colder. Soon the balloon stops floating higher and begins sinking. Assuming that there is no air loss, which of the following is the best explanation for this observation? A) The difference in temperature between the air inside and outside the balloon produces convection currents, which lose strength at high altitude. B) The air density inside the balloon has become greater than the surrounding air density. C) The cooler air outside the balloon pushes in on the walls of the balloon. D) The pressure on the walls of the balloon decreases with decreasing temperature.
B
At 25°C He gas (molar mass 4.00 grams) effuses at a rate of 0.100 mole per minute. What is the rate of effusion of O2 (molar mass 32.0 grams)? A) 0.025 mole per minute B) 0.035 mole per minute C) 0.10 mole per minute D) 0.20 mole per minute
B
Base your answer to the following question on the following types of energy. (A) Lattice Energy (B) Ionization Energy (C) Activation energy (D) Hydration energy The minimum amount of energy required to remove the most loosely held electron of an isolated gaseous atom. A) A B) B C) C D) D
B
Equal numbers of moles of H2O(g), F2(g), Cl2(g) are placed into a single container. The container has a pinhole-sized leak (1 mm), and after 10 minutes some gas has escaped from the container. What is best reason for why there is more Cl2 gas left in the container than any other gas? (NOTE: the molecules do not react with each other) A) The Cl2 molecule is too big to escape through the leak-hole B) The rate of effusion for Cl2 is less than than that of the other two gases C) Cl2 is a nonpolar molecule D) H2O has the greatest rate of diffusion
B
In 1811 Avogadro calculated the formula of camphor by means of elemental chemical analysis and by measuring the density of its vapor. Avogadro found the density to be 3.84 g/L when he made the measurements at 210°C at 1 atmosphere pressure. Which of the following is the correct formula for camphor? A) C10H14O B) C10H16O C) C10H16O2 D) C10H18O
B
The gaseous pressure in a 500 mL flask is 250 mmHg at 284 K. What is the number of moles of gas present in the flask? A) 0.00143 mole B) 0.00705 mole C) 7.05 moles D) 143 moles
B
The pressure of a real gas is sometimes less than that predicted by the ideal gas law because the ideal gas law does not include the factor of A) mass of molecules B) intermolecular forces C) size of molecules D) energy of molecules
B
The temperature of a sample of H2O(l) in a closed container is decreased. Which of the following can be true? A) Volume constant, pressure increased, density constant B) Volume constant, pressure decreased, density constant C) Volume decreased, pressure constant, density increased D) Volume decreased, pressure increased, density decreased
B
The temperature of a sample of xenon atoms is raised from 50oC to 90oC. Which of the following statements is true about the average kinetic energy of the atoms? A) The average kinetic energy does not change. B) The average kinetic energy of the sample increased by a factor of 363/323. C) The average kinetic energy of the sample increased by a factor of 9/5. D) The average kinetic energy increased by a factor of 81/25.
B
The weight of HC2H3O2 (molecular weight 60.0) in 20.0 milliliters of a 2.50-molar solution is A) 2.50 grams B) 3.00 grams C) 6.00 grams D) 30.0 grams
B
What is the density of oxygen gas at STP? A) 0.7 g/L B) 1.4 g/L C) 2.5 g/L D) 32. g/L
B
What is the percent composition of a solution where 60. g of a 10% salt solution in water is mixed with 40. g of a 20% solution of the same salt? All are mass percents A) 8% B) 14% C) 15% D) 16%
B
What is the vapor pressure of a 20.0% by mass solution of C6H14NO5 (molar mass 180.) in water at 29°C (vapor pressure of pure water at 29.0°C is 30.0 torr)? A) 0.700 torr B) 29.3 torr C) 30.0 torr D) 70.0 torr
B
Which of the following aqueous solutions has the lowest freezing point? A) 0.10 M Magnesium Chloride: MgCl2 B) 0.10 M Sodium Phosphate: Na3PO4 C) 0.10 M Lithium Chloride: LiCl D) 0.10 M Hydrobromic acid: HBr
B
"The pressure of a given mass of gas varies directly with the absolute, Kelvin, temperature with the volume being kept constant." This statement best illustrates A) Boyle's Law B) Combined Gas Law C) Gay-Lussac's Law D) Charles' Law
C
2 Li + 2 H2O 2 Li+ + 2 OH- + H2 When 0.800 mol of Li is reacted with excess water at STP in the equation above, what volume of hydrogen gas is produced? A) 4.48 L B) 6.72 L C) 8.96 L D) 17.92 L
C
A 0.821 L container at 273 C contains 10.0 moles of neon gas. What is the pressure inside the container? A) 410. atm B) 137. atm C) 546. atm D) 273. atm
C
A 50.0 mL aliquot of a sulfuric acid solution was treated with barium chloride and the resulting BaSO4 was isolated and weighed. If 0.667 g of BaSO4 was obtained, what was the molarity of the H2SO4? A) 0.00700 M B) 0.0286 M C) 0.0572 M D) 0.114 M E) 1.43 M
C
A gaseous mixture contains 4.50 moles hydrogen, 2.50 moles oxygen, and 3.00 moles argon. This system exerts a total pressure of 0.500 atmosphere. What is the partial pressure of the hydrogen? A) 0.025 atm B) 0.135 atm C) 0.225 atm D) 0.356 atm
C
A plastic bag is massed. It is then filled with a gas which is insoluble in water and massed again. The apparent weight of the gas is the difference between these two masses. The gas is squeezed out of the bag to determine its volume by the displacement of water. What is the actual weight of the gas? A) .90 g B) 1.92 g C) 2.82 g D) 3.90 g
C
A sealed metal tank is filled with neon gas. Which of the following does NOT occur when neon gas is pumped into the tank at a constant temperature? (A) The average speed of the neon atoms remains the same. B) The average distance between molecules decreases. C) The volume of the gas decreases. D) The pressure inside the tank increases.
C
A solution of MgCl2has a chloride ion concentration of 0.300 M, what is the concentration of MgCl2? A) 0.300 M B) 0.200 M C) 0.150 M D) 0.100 M
C
A student collected a sample of gas using water displacement. Which of the following measurements is necessary to determine the vapor pressure of the water in the sample? A) The kinetic energy of the gas B) The volume of the water C) The temperature of the water D) The water solubility of the gas
C
A student raises the temperature of an aqueous solution of KBr from 313K to 363K. Which of the following statements is true? A) The normality of the solution decreases. B) The molarity of the solution remains the same. C) The solution's molality does not change. D) The density of the solution does not change.
C
As the concentration of HCl in aqueous solution increases, which of the following decreases? A) Osmotic pressure B) Temperature C) Freezing point D) Electrical conductivity
C
BCl3NH3 BCl3 + NH3 A student places 0.10 mole of BCl3NH3 in a 1 L vacuum flask, which is sealed and heated. The BCl3 NH3 decomposes completely according to the balanced equation above. If the flask's temperature is 375. K, the total pressure in the flask is closest to which of the following? (Use R = 0.08 L•atm/mol•K) A) 6.0 atm B) 1.5 atm C) 3.0 atm D) 7.5 atm
C
Base your answer to the following question on the following types of energy. (A) Lattice energy (B) Potential energy (C) Kinetic energy (D) Electromagnetic energy Energy that is measured by 1/2mv^2 A) A B) B C) C D) D
C
C3H7OH (s) H2O(g) + C3H6 (g) A student places 0.05 mole of C3H7OH (s) in a 1 L vacuum flask, which is sealed and heated. The propanol decomposes completely according to the balanced equation above. If the flask's temperature is 500. K, the total pressure in the flask is closest to which of the following? (Use R = 0.08 L•atm/mol•K) A) 50. atm B) 25. atm C) 2.0 atm D) 4.0 atm
C
How many milliliters of 11.5-molar HCOOH must be diluted to obtain 23 L of 2.0-molar HCOOH? A) 1000 mL B) 3000 mL C) 4000 mL D) 5000 mL
C
How much water must be added to 300. mL of a 7.00 M HCl solution to reduce the concentration to 4.20 M? A) 50.0 mL B) 150. mL C) 200. mL D) 400. mL
C
Hydrogen gas is collected over water at 29oC. The total pressure of the system is 773 torr. If the vapor pressure of water at 29oC is 30 torr, what is the partial pressure of the hydrogen gas? A) 803 torr B) 30 torr C) 743 torr D) 773 torr
C
Potassium Chloride, KCl, is less effective than an equal mass of sodium chloride, NaCl, for raising the boiling point of water because A) KCl is less soluble in water than NaCl. B) KCl(s) has a lower boiling point than NaCl(s). C) KCl has a larger formula mass than NaCl. D) NaCl forms hydrogen bonds and KCl does not.
C
Samples of F2 and Kr gas are mixed in a rigid container. The initial partial pressure of fluorine is 1.2 atm and the partial pressure of the krypton is 0.2 atm. After all the krypton reacted, forming a solid compound, the total pressure was 0.7 atm. What is the formula for this compound? A) KrF B) Kr2F5 C) KrF5 D) KrF7
C
The weight of HNO3 (molecular weight 63.0) in 40.0 milliliters of 5.00-molar solution is A) 5.6 g B) 10.4 g C) 12.6 g D) 13.1 g
C
Under what conditions do gases deviate the most from ideal behavior? A) High temperature, low pressure B) Low temperature, low pressure C) Low temperature, high pressure D) High pressure only
C
What is the concentration of ammonium ions in a 0.100 M solution of (NH3)2SO4? A) 0.020 M B) 0.100 M C) 0.200 M D) 0.300 M
C
What is the molarity of concentrated HCl? A) 0.82 M B) 3.3 M C) 9.87 M D) 12.5 M
C
What is the percent by mass of NH3CO3 (molar mass 77. g) in a 2.0 M solution that has a density of 1.1 g/mL? A) 1.4% B) 2.6% C) 14.% D) 26.%
C
What is the total pressure after 1.00 mole of H2(g), 1.00 mole of N2(g), 1.00 mole of O2(g) and 3.00 moles of CO2(g), are injected into a rigid 22.4 L container at 273 K? A) 760 mmHg B) 2,280 mmHg C) 4,560 mmHg D) 9,120 mmHg
C
Which of the following dissolves in water to form an ionic solution? A) O2 B) SiO2 C) KMnO4 D) C12H22O11
C
Which of the following would have the highest boiling point? A) a 1.5 M solution of AlCl3 B) a 2.0 M solution of NaCl C) a 2.5 M solution of Na2S D) a 3.0 M solution of HCl
C
Why does a 1-molal solution of table salt (NaCl) have a lower freezing point than a 1-molal solution of sugar (C6H12O6)? A) Molecules of table salt are smaller than the molecules of sugar. B) Molecules of table salt have stronger bonds than molecules are sugar. C) Table salt is ionic and dissociates in water, sugar does not. D) Solid table salt has a different crystalline structure than sugar.
C
A 2.70 L sample of nitrogen gas is kept at a pressure of 800. torr and 27.0°C. what would its volume be if the pressure was increased to 1200. torr and it was cooled to -73.0°C. A) 1.80 L B) 2.70 L C) 3.60 L D) 1.2 L
D
A clear, colorless liquid in a beaker in a hood is heated at a constant rate. The liquid begins to boil at 110°C. The boiling temperature gradually increases to 115°C, at which time the heating is discontinued. The material in the beaker is probably a A) pure element B) pure compound C) heterogeneous solution D) homogeneous solution
D
A gas has a density of 0.25 g/L at a pressure of 0.0821 atm and a temperature of 27. C. What is the molar mass of the gas? A) 0.25 g/mol B) 30. g/mol C) 38. g/mol D) 75. g/mol
D
A rigid cylinder is filled with gas. At constant temperature, which of the following applies to the gas in the cylinder when gas is released? A) The average kinetic energy of the gas particles increases. B) The pressure of the gas increases. C) The total number of gas molecules stays constant. D) The total force of the gas molecules hitting the side of the container decreases.
D
A solution of a nonvolatile molecular solute in benzene is prepared. Which describes what happens to the freezing point, boiling point, and vapor pressure of the solution compared to pure benzene? A) Freezing point and boiling point increase, vapor pressure decreases B) F.P. decreases, V.P. and B.P. increase C) F.P. and V.P. increase, B.P. decreases D) F.P. and V.P. decrease, B.P. increases
D
At 25.°C, C2H6 (molar mass 30. g) effuses at a rate of 0.38 mole per minute. Which gas would have a rate of effusion approximately one-half as fast? A) CH4 (molar mass 16. g) B) NO (molar mass 30. g) C) N2O3 (molar mass 76. g) D) Cl2O3 (molar mass 119. g)
D
Base your answer to the following question on the types of solids given below. (A) A molecular solid with hydrogen bonds (B) A molecular solid with non-polar molecules (C) A network solid (D) An ionic solid For solutions of equal molality, which would generally have the greatest freezing point depression? A) A B) B C) C D) D
D
Equal numbers of moles of CO2(g), NH3(g), SO2(g) are placed into 3 separate identical containers. If each container has an identical pinhole leak, which of the following is true about the moles of gas remaining in each container after some time has elapsed? A) mol CO2 < mol NH3 < mol SO2 B) mol CO2 < mol SO2 < mol NH3 C) mol NH3 < mol SO2 < mol CO2 D) mol NH3 < mol CO2 < mol SO2
D
Find the partial pressure of Hydrogen gas collected over water at 18oC if the the vapor pressure of water at 18oC is 15.5 torr, and the total pressure of the sample is 745 torr. A) 760.5 torr B) 745.0 torr C) 15.5 torr D) 729.5 torr
D
How many milliliters of 4.5-M H2CO3 must be diluted to obtain 12.0L of 3.0-M H2CO3? A) 2000 mL B) 2500 mL C) 4000 mL D) 8000 mL
D
If 149 grams of Ca(OH)2 is dissolved in 500 mL of water, what are the resulting concentrations of calcium 2+ and hydroxide ions? Ca2+ OH- A) 2 M 2 M B) 4 M 4 M C) 8 M 4 M D) 4 M 8 M
D
The density of air at STP is 1.29 gL-1 and that of oxygen is 1.43 gL-1. The specific gravity of oxygen, using air as the standard, is found by A) (1.29 gL-1) + (1.43 gL-1) B) (1.29 gL-1) x (1. 43 gL-1) C) (1.43 gL-1) - (1.29 gL-1) D) (1.43 gL-1) / (1.29 gL-1)
D
What is the density of a 1.0 M solution of C5H10O2 that is 7.5% C5H10O2 by mass? A) 1.0 g/mL B) 0.50 g/mL C) 1.5 g/mL D) 1.4 g/mL
D
What is the molarity of a solution of NaF that is 14.% solute by mass and has a density of 1.20 g/mL? A) 0.50 M B) 1.0 M C) 3.0 M D) 4.0 M
D
When 110. grams of Mg(ClO4)2 (molar mass of 220. g) is dissolved in enough water to make 500. milliliters of solution, what are the concentrations of the Mg2+ and ClO4- ions respectively? A) 0.500 M and 1.00 M B) 1.00 M and 1.00 M C) 1.00 M and 0.500 M D) 1.00 M and 2.00 M
D
When 228. g of K2C2O2 (molar mass 144. g) is dissolved in enough water to make 500.mL of solution, what are the concentrations of the K+ and C2O22- ions respectively? A) 2.00 M and 4.00 M B) 4.00 M and 4.00 M C) 4.00 M and 8.00 M D) 8.00 M and 4.00 M
D
Which of the following is NOT an assumption of the ideal gas law A) All collisions are elastic B) All gases behave in the same manner C) Particles are sizeless D) There is no effect of the kinetic energy of particles on the equation of state
D
Base your answers to questions 12 through 14 on a balloon containing 35.5 grams of Cl2(g) and 38.0 grams of F2(g). If the balloon is punctured, which gas will leak out faster?
F
A 5.67 gram sample of iodine heptafluoride is placed in a 3.0 liter evacuated flask and completely vaporized at 184C. (a) If no reaction occurs, what is the pressure in the flask. (b) Iodine heptafluoride decomposes according to the reaction IF7 IF5 + F2 If the pressure in the flask is measured to be .50 atmospheres, what is the partial pressure of the IF7 and the IF5 at 184C.
a. .273 atm b. IF7 = .046 IF5 = .227 atm
Give a scientific explanation for each of the following observed phenomena. (a) A hydrogen filled balloon can lift more weight than a helium filled balloon of equal volume. (b) When a balloon filled with gas is allowed to sit undisturbed, its volume slowly decreases.
a. hydrogen is less than helium b. gas effuses through the walls of the balloon
If the volume is increased to 10 L and the temperature is kept constant, calculate the following. i. Mole fraction of Cl2(g). ii. The partial pressure of Cl2(g).
i. .33 ii. 1.22
