When must temperature values in gas law calculations be expressed in kelvin units?
A) only for Charles's law
B) only for the Ideal Gas law
C) only for the Combined Gas law
D) never
E) always
Answer: E
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Chemistry Chapter 11
- What is the volume of 28.0 g of nitrogen gas at STP?
- What is the pressure of a 1.0 L flask containing 0.60 g of He at 25°C? (R= 0.0821 L atm/ mol K)
- What is the molecular weight of a gas if a 21.0 g sample has a pressure of 836 mm Hg at 25.0°C in a 2.00 L flask? (R= 0.0821 L atm/ mol K)
- What is the volume (in liters) of 1.00 mole of krypton gas that has a pressure of 1140 mm Hg and a temperature of 25.0°C? (R= 0.0821 L atm/ mol K)
- If the number of moles of a gas initially contained in a 2.10 L vessel is doubled, what is the final volume of the gas in liters? (Assume the pressure and temperature remain constant.)
- A rigid cylinder contains 2.00 liters of gas at a temperature of 25°C. If the pressure of this gas is changed from 0.500 atmospheres to 1.50 atmospheres, what will be the new temperature (in Kelvin, reported to three significant figures) of the gas? (The volume is constant.)
- What is the final pressure (expressed in atm) of a 3.05 L system initially at 724 mm Hg and 298 K, that is compressed to a final volume of 2.51 L at 273K?
- What is the final volume (L) of a 1.00 L system at 315 K and 1.10 atm if STP conditions are established?
- What is the change in temperature of a 2.50 L system when its volume is reduced to 1.75 L if the initial temperature was 298 K?
- What is the final volume of a gas that initially occupies 2.50 L at 298 K and is subsequently heated to 321 K?
- What is the final volume (L) of a 10.0 L system that has the pressure quartered?
- What is the final pressure of a system (atm) that has the volume increased from 0.75 L to 1.1 L with an initial pressure of 1.25 atm?
- What is the pressure of 760 mm Hg when expressed in units of in Hg?
- How many liters of O2 (g) are needed to react completely with 56.0 L of CH4 (g) at STP to produce CO2 (g) and H2O (g)?
- Water can be formed according to the equation 2H2 (g) + O2 (g) ? 2H2O (g) If 8.0 L of hydrogen is reacted at STP, exactly how many liters of oxygen at STP would be needed to allow complete reaction?
- If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?
- Suppose you had a balloon containing 1 mole of helium at STP and a balloon containing 1 mole of oxygen at STP. Which statement is TRUE?
- At STP, 12.69 g of a noble gas occupies 14.09 L. What is the identity of the noble gas? (R= 0.0821 L atm/ mol K)
- Which set of conditions reflect STP?
- Suppose a chemical reaction generated a 50% nitrogen/50% oxygen (by volume) mixture of gas that had a total volume of 22.4 liters at STP. This gas sample is composed of
- Hydrogen gas produced in the laboratory by the reaction of zinc and hydrochloric acid was collected over water at 25°C. The barometric pressure at the time was 742.5 mm Hg. What is the pressure of dry hydrogen gas if the vapor pressure of water at 25°C is 23.8 mm Hg?
- The vapor pressure of water at 20.0°C is 17.5 mm Hg. If the pressure of a gas collected over water was measured to be 453.0 mm Hg. What is the pressure of the pure gas?
- Human lungs have evolved to breathe oxygen at a pressure as that in the atmosphere, 0.21 atm. If a particular heliox mixture to be carried by a scuba diver is at a pressure of 7.00 atm, what should be the partial pressure due to helium in order to maintain the pressure due to oxygen at 0.21 atm?
- What problem could happen if deep sea divers used pure oxygen in their tanks?
- A "shielding gas" mixture of argon and carbon dioxide is sometimes used in welding to improve the strength of the weld. If a gas cylinder of this two-part mixture was at 4.0 atm pressure and this mixture was 90.% argon, what would be the pressure due to the carbon dioxide gas component?