Ideal Gas Law
What is the ideal gas constant equal to?
R = 0.08206 L atm/mol K
(8.134 J/mol K)
When the formation of a compound gives off heat is this an Exothermic or Endothermic reaction?
Exothermic
D = g/L
In a flask filled with gas, what will Ptotal be equal to?
Ptotal - PA + PB + PC ...
How do you calculate partial pressure?
Ppartial = XNe / (Xtotal)
What is the ideal gas constant equal to?
R = 0.08206 L atm/mol K
(8.134 J/mol K)
What is the equation used to determine bond enthalpy?
Hrxn = BE(reactants) - BE(products)
(Breaking - Making)
A 0.807 gram sample of an unknown gas is found to occupy a volume of 1.05 L at a pressure of 391 mm Hg and a temperature of 52 °C. The molecular weight of the unknown gas is?
M = 39.8 g/mol
A mixture of argon and neon gases, in a 5.98 L flask at 19 °C, contains 13.5 grams of argon and 3.04 grams of neon. What is the partial pressure of neon in the flask, and the total pressure of gas in the flask?
PNe = 0.604 atm Ne
Ptotal = 1.96 atm
A mixture of xenon and argon gases, at a total pressure of 625 mm Hg, contains 12.9 grams of xenon and 2.40 grams of argon. What is the partial pressure of each gas in the mixture?
PAr = 237 mm Hg
PXe = 388 mm Hg
It is desired to inflate a baggie with a volume of 986 mL by filling it with O2 gas at a pressure of 1.05 atm and a temperature of 297 Kelvin. How many grams of O2 gas are needed?
1.36 grams
Determine the bond enthalpy for the following reaction: 2H2 + O2 = 2H2O
-482 kJ/mol
A common organic solvent used in the laboratory vaporizes readily. If the pressure of the compound's vapor in a flask is 214 mmHg at 25 °C, and the density of the vapor is 0.669 g/L, what is the molar mass of the compound?
M = 58.08 g/mol
The stopcock connecting a 4.36 L bulb containing nitrogen gas at a pressure of 9.56 atm, and a 9.37 L bulb containing oxygen gas at a pressure of 1.02 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is?
P = 3.73 atm
Name the three additional gas laws and the equation for each.
Avogadro's: V1/n1 = V2/n2
Boyle's: P1V1 = P2V2
Charles's: V1/T1 = V2/T2
A 1.34 mol sample of krypton gas at a temperature of 29.0 *C is found to occupy a volume of 21.4 L. What is the pressure of this gas sample in mm Hg?
1.18 x 103 mm Hg
Determine the bond enthalpy for the following reaction: 2HCl + Br2 = 2HBr + Cl2
+83 kJ/mol
What is the density of a sample of hydrogen gas at a pressure of 1.09atm and a temperature of 35*C?
D = 8.69 x 10-2 g/L
A mixture of nitrogen and oxygen gases is maintained in a 9.20 L flask at a pressure of 3.84 atm and a temperature of 84.0 °C. If the gas mixture contains 6.82 grams of nitrogen, the number of grams of oxygen in the mixture is?
30.8 g of O2
A mixture of neon and methane gases contains neon at a partial pressure of 408 mm Hg and methane at a partial pressure of 328 mm Hg. What is the mole fraction of each gas in the mixture?
XCH4 = 0.446
At what temperature (*C) would one liter of boron trifluoride gas have a mass of 2.698g, if the gas pressure is 0.813atm?
-24.0 *C
Determine the bond enthalpy for the following reaction: 2C3H6 + 9O2 = 6CO2 + 6H2O
-2.93 x 103 kJ/mol
A sample of an unknown gas is found to have a density of 0.769 g/L at a pressure of 0.514 atm and a temperature of 52 °C. Assume ideal behavior.
M = 39.9 g/mol
The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 756 mm Hg. If the wet H2 gas formed occupies a volume of 9.72 L, the number of grams of H2 formed is?
(The vapor pressure of water is 23.8 mm Hg at 25 °C.)
0.772g H2
How many grams of iron are needed to completely consume 6.46 L of oxygen gas according to the following reaction at 25 °C and 1 atm?
iron (s) + oxygen (g) = iron(ll) oxide (s)
29.5 g of Fe