The Ideal Gas Laws assignment and quiz

Consider a balloon with volume V. It contains n moles of gas and has an internal pressure of P. The temperature of the gas is T. The balloon is placed in a freezer at temperature 0.75T. The freezer is pressurized at 1.25P. Which of these could be the final volume of the balloon? The balloon is removed from the freezer and returned to its initial conditions. It is then heated to a temperature of 2T at a pressure of 2P. How does the volume of the balloon change? If the number of moles of gas increases to 1.5n, what is the new volume if pressure and temperature are held constant?

0.60V It does not change. 1.5V

A balloon containing 0.500 mol Ar at 0.00°C and 65.0 kPa pressure is expanded by adding more argon. How many moles of argon are added to bring the sample to a final volume of 60.0 L at 30.0°C and 45.0 kPa? What is the original volume of the gas? How many moles of argon exist in the new conditions? How many moles of argon were added?

17.5 L 1.07 mol 0.570 mol

What is the temperature of 0.750 mol of a gas stored in a 6,850 mL cylinder at 2.21 atm? Use mc032-1.jpg and mc032-2.jpg. 2.95 K 5.24 K 138 K 246 K

246 K

What is the pressure of 0.540 mol of an ideal gas at 35.5 L and 223 K? Use mc031-1.jpg and mc031-2.jpg. 0.715 kPa 2.45 kPa 28.2 kPa 62.7 kPa

28.2 kPa

What is the temperature of 0.80 mol of a gas stored in a 275 mL cylinder at 175 kPa? Use mc026-1.jpg and mc026-2.jpg. 4.6 K 7.2 K 61 K 96 K

7.2 K

Which laws can be combined to form the ideal gas law? Boyle's law and Charles's law Gay-Lussac's law and Avogadro's law Charles's law, Avogadro's law, and Boyle's law Dalton's law, Gay-Lussac's law, and Avogadro's law

Charles's law, Avogadro's law, and Boyle's law

A gas has experienced a small increase in volume but has maintained the same pressure and number of moles. According to the ideal gas law, how has the temperature of the gas changed? It has increased two times. It has increased slightly. It has decreased slightly. It has stayed the same.

It has increased slightly.

Consider a balloon that has a volume V. It contains n moles of gas, it has an internal pressure of P, and its temperature is T. If the balloon is heated to a temperature of 15.5T while it is placed under a high pressure of 15.5P, how does the volume of the balloon change? It doubles. It stays the same. It increases greatly. It decreases slightly.

It stays the same.

If the pressure of a 2.00 L sample of gas is 50.0 kPa, what pressure does the gas exert if its volume is decreased to 20.0 mL? Which equation should you use? What is the new pressure?

P1V1 = P2V2 5000 kPa

At 35.0°C and 3.00 atm pressure, a gas has a volume of 1.40 L. What pressure does the gas have at 0.00°C and a volume of 0.950 L? Which equation should you use? What is the pressure of the gas?

P2 = P1V1T2/T1V2 3.92 atm

What is the temperature in kelvin of a gas if it is allowed to expand from 1.50 L to 4.50 L? The initial temperature is 10.0°C and pressure is constant throughout the change. Which equation should you use? What is the final temperature?

T2 = V2T1/V1 849 K

Which equation agrees with the ideal gas law?

V1/T1 = V2/T2

Identify all of the gas law equations that relate to the ideal gas law.

V1/T1 = V2/T2 V1/n1 = V2/n2 P1V1 = P2V2 P1/T1 = P2/T2

Which law relates to the ideal gas law?

V1/n1 = V2/n2

A sample of N2 gas occupying 800.0 mL at 20.0°C is chilled on ice to 0.00°C. If the pressure also drops from 1.50 atm to 1.20 atm, what is the final volume of the gas? Which equation should you use? What is the final volume of the gas?

V2 = P1V1T2/P2T1 932 mL

A balloon containing 0.0400 mol of a gas with a volume of 500 mL was expanded to 1.00 L. Answer the questions and round answers to nearest hundredth place. Which equation should you use to find the amount of gas added? What is the final number of moles?

b. n2 = V2n1/V1 0.08 moles

Consider the proportionality below. mc009-1.jpg What does this best represent? Dalton's law Charles's law ideal gas law combined gas law

ideal gas law

Which law relates temperature, pressure, volume, and the number of moles of a gas under perfect conditions? Boyle's law Charles's law ideal gas law combined gas law

ideal gas law

Determine the number of moles of air present in 1.35 L at 750 torr and 17.0°C. Which equation should you use? What is the number of moles present?

n = PV/RT 0.056 mol