Initially, a sealed balloon filled with helium gas at 20.0 °C occupies 2.91 L at 1.00 atm. The balloon is then immersed in liquid nitrogen at −196 °C, raising the pressure to 5.20 atm. What is the volume (in L) of the balloon in the liquid nitrogen? Group of answer choices 3.98 L 0.000669 L 5.48 L 0.147 L 2.13 L
Initially, a sealed balloon filled with helium gas at 20.0 °C occupies 2.91 L at 1.00...
A balloon filled with helium gas at 20C occupies 2.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196C, raising the pressure to 5.20 atm. What is thevolume of the balloon in the liquid nitrogen?Please explain how you solve this.
A balloon filled with helium gas at 1.00 atm occupies 9.3 L. What volume in liters will the balloon occupy in the upper atmosphere, at a pressure of 0.46 atm?
A balloon filled with helium gad at 1.00 atm occupies 15.5 L. What volume would the balloon occupy in the upper atmosphere, at a pressure of 0.25 atm and a constant temperature?
Helium gas in a balloon occupies 2.5 L at 300.0 K. The balloon is dipped into liquid nitrogen that is at a temperature of 80.0 k. What will the volume of the helium in the balloon at the lower temperature be? I got a weird answer like .66667 and i used charles law
A helium-filled balloon at 1.00 atm pressure has a volume of 1.200 L. It is placed in a freezer and its volume decreases, stopping at 1.010 L. (Assume that the static internal and external pressures are equal, that the balloon contains only helium, and helium behaves as an ideal gas.) Calculate ΔE for the gas in the balloon.
A helium-filled balloon at 1.00 atm pressure has a volume of 1.320 L. It is placed in a freezer and its volume decreases, stopping at 0.990 L. (Assume that the static internal and external pressures are equal, that the balloon contains only helium, and helium behaves as an ideal gas.) Calculate ΔE for the gas in the balloon.
A balloon filled with 2.00 L of helium initially at 1.35 atm of pressure rises into the atmosphere. When the surrounding pressure reaches 500. mmHg, the balloon will burst. If 1 atm = 760. mmHg, what volume will the balloon occupy in the instant before it bursts?
A balloon filled with 35.6 moles of helium has a volume of 856 L at 0.0°C and 1.00 atm pressure. The temperature of the balloon is increased to 43.0°C as it expands to a volume of 967 L, the pressure remaining constant. Calculate q, w, and ΔE for the helium in the balloon. (Given, the molar heat capacity for helium gas is 20.8 J/°C · mol, and 1 L·atm = 101.3 J) (Show your work)
1. A helium-filled weather balloon has a volume of 558 L at 22.9°C and 751 mmHg. It is released and rises to an altitude of 3.13 km, where the pressure is 582 mmHg and the temperature is 1.9°C. The volume of the balloon at this altitude is ____L. 2. A sample of helium gas collected at a pressure of 1.42 atm and a temperature of 17.0 °C is found to occupy a volume of 22.9 liters. How many moles of...
QUESTION 4 A 0.973 mole sample of helium gas at 25 C filled a balloon to a volume of 3.87 L. What is the pressure of the balloon? 6.15 atm 1.12x103 atm 74.9 atm 0.516 atm