SLO 6 (Gas Laws)
The percent by mass of bicarbonate (HCO3−) in a certain Alka-Seltzer product is 32.5 percent. Calculate the volume of CO2 generated (in mL) at 37 °C and 1.00 atm if a person were to accidentally ingest a 3.15-g tablet without following instructions. (Hint: The reaction occurs between HCO3− and HCl acid in the stomach.)
(Enter your answer in scientific notation)
(a) ____________ : at constant ____________ , the ____________ occupied by a fixed amount of gas is ____________ proportional to its absolute ____________ . (b) ____________ : at fixed ____________ and pressure, the ____________ occupied by a gas is ____________ proportional to the ____________ . (c) ____________ : at constant ____________ , the ____________ occupied by a fixed amount of gas is ____________ proportional to the applied (external) ____________ .
(a) Charles's law, pressure, volume, directly, temperature (b) Avogadro's law, temperature, volume, directly, number of moles (c) Boyle's law, temperature, volume, inversely, pressure
(a) Directly Proportional (b) Inversely Proportional
(a) Density & molar mass, Volume & number of moles, Volume & absolute temperature, Pressure & absolute temperature, Pressure & number of moles (b) Volume & pressure
What volumes (in liters) of carbon monoxide and oxygen gas must react according to the equation 2CO(g) + O2(g) → 2CO2(g) to form 2.96 L of carbon dioxide? (a) What is the volume of CO? (b) What is the volume of O2?
(a) L (b) L
A 58−L sample of dry air cools from 184 °C to −41 °C while the pressure is maintained at 2.91 atm. What is the final volume?
L
A gas-filled balloon with a volume of 3.00 L at 1.20 atm and 20°C is allowed to rise to the stratosphere (about 30 km above the surface of the Earth), where the temperature and pressure are −23°C and 3.00 × 10−3 atm, respectively. Calculate the final volume of the balloon.
L
What is the volume of 5.37 moles of an ideal gas at 35.5 °C and 1.00 atm?
L
Find the density of Freon−11 (CFCl3) at 172 °C and 2.55 atm
M = drt/p M = molecular mass of substance d = density of gas r = gas constant (atm = 0.08206) t = Temperature in K We just find out that Freon-11's molecular mass is: C = 12 F = 19 Cl = 35.5 12+19+(3*35.5) = 137.5 = M (in the equation) R = 0.08206 T = 445.15 K (to convert into kelvin, just add 273.15 to the Celsius) P = 2.55 atm d = ? 137.5 = (d x 0.08206 x 445.15)/2.55 d = g/L
A 89.6−g sample of dinitrogen monoxide is confined in a 3.54−L vessel. What is the pressure (in atm) at 106 °C?
atm
At what pressure would a sample of gas occupy 7.06 L if it occupies 2.64 L at 4.66 atm? (Assume constant temperature.)
atm
At −11 °C a sample of carbon monoxide gas exerts a pressure of 0.33 atm. What is the pressure when the volume of the gas is reduced to one-third of the original value at the same temperature?
atm
A sample of sulfur hexafluoride gas occupies 6.86 L at 212 °C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 1.78 L?
°C
At what temperature (in °C) would 1.00 mole of ideal gas occupy 75.0 L (P = 1.00 atm)?
°C
