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A: Volume, V = 515 cm3 mass, m = 0.460 g Pressure, P = 153 kPa temperature, T = 322 K
Q: 1.1. Compute the density (in units of m) of an ideal gas under the following conditions: (a) At 0 °C…
A: Ans:- Image-1
Q: Dry air is 78.1% nitrogen. What is the partial pressure of nitrogen when the atmospheric pressure is…
A: atmospheric pressure is 1.01 X 105 N/m2
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A: Initial volume of ideal gas = 6 L Initial temperature = 375 k final temperature = 175 k Initial…
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A: In order to define how gases expand when they gets heated is by using the Charles law. This says
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A: The partial pressure of nitrogen in the atmosphere, P=79.11 kPa
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Q: What is gas density, if under pressure of 105 Pa, its molecules move at a speed of 300 m/s?
A: The formula for the pressure in terms of volume and density is:
Q: Find the number of moles in 6.00 L of gas at 20.0°C and under 7.04 ✕ 107 N/m2 of pressure.
A: Pressure, P= 7.04 x 107 Pa Volume, V = 6 L=6 x 10-3 m3 Temperature, T = 20°C = 293 K
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A: Given: Pressure P = 350 kPa Temperature T = 20 ℃ =(273+20)K = 293 °K Gas constant R = 0.462…
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Q: The density of air at 0⁰C and 1 atm pressure is 1.293 Kg/m³. What is its density at a pressure of 2…
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A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…
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Q: At standard temperature and pressure, a gas has a density of 0.089 kg/m3. What volume (in m3) does…
A: The density of the gas: ρ = 0.089 kg/m3; The mass of the hydrogen gas: m = 1.84 kg;
Q: What is the pressure of a 3.00-mol gas whose temperature is 60.0 oC and whose volume is 5.00 L?
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A: Given:- The gas initially at STP V1 = 3 m3 P2 = 2 atm The temperature of the gas rises to 22◦C…
If a gas occupies 250 cm3 at 37oC. What is its volume at 67oC if the pressure changed from 1.5 atm to 1 atm?
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- The temperature of an ideal gas remains constant while the pressure changes from 103.425 Kpaa to 1034.25 Kpaa. (a) If the initial volume is 0.08 cubic meters, determine the final volume. (b) For 0.77 Kgm of this gas, determine the change in density as a percentage of the initial density.How many moles of an ideal gas are there if the volume of the gas is 158L at 14°C and a pressure of 89 kPa?A cylinder is filled with10.0Lof gas and a piston is put into it. The initial pressure of the gas is measured to be 268.kPa.The piston is now pushed down, compressing the gas, until the gas has a final volume of 8.70L. Calculate the final pressure of the gas. Round your answer to 3 significant digits.
- What is the volume of 67 mol of gas, in the unit of m3, when the pressure is 87 kPa and the temperature is 68°C? Use R = 8.314 J/(K mol) for the gas constant. Be careful with units, and remember that the temperature must be in Kelvin when you use the ideal gas equation.How many moles of gas are in a bike tire with a volume of 2.00×10 – 3 m3(2.00 L), a pressure of 7.00×105 Pa (a gauge pressure of just under 90.0 lb/in2 ), and at a temperature of 18.0ºC ?What is the gauge pressure of a 0.04 m³ tank holding 107 g of argon gas at 20 C? The molecular weight of argon is 40 g/mol, and atmospheric pressure is 101.3 kPa. Answer in kPa.
- If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0 C, what is the volume of the container that the gas is in?What is the molar mass of a gas if 1.30g of the gas has a volume of 255 mL at STP? ( THE ANSWER IS NOT 130g/mol)Macroscopic Description of an Ideal Gas. An auditorium dimension 10 m x 20 m x 30 m. How many molecules of air fill the auditorium at 20.00and a pressure of 101 kPa?
- A gas is held in a container with volume 516 cm3. If the pressure of the gas inside the container is 100 kPa, what is the pressure of the gas, in the unit of kPa, when it is expanded to 733 cm3? Assume that the temperature of the gas does not change.Four moles of an ideal gas are confined to a 35-liter container at a temperature of 30ºC. What is the pressure of the gas in atm? (hint: check units) a) 0.828 atm b) 2.84 atm c) 28.4 atm d) 288 atm5.0 moles of an ideal gas are confined to a 15-liter container at a pressure of 2.6x105 Pa. What is the temperature of the gas?