Gas behave most ideally at low pressures, low temperatures high pressures, high temperatures high pressure, low...
Gas behave most ideally at
low pressures, low temperatures
high pressures, high temperatures
high pressure, low temperatures
low pressures, high temperatures
Homework Answers
Answer: low pressures, high temperatures
Because at these condition, molecules move fast and the potential energy between molecules becomes least significant.
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Gas behave most ideally at
low pressures, low temperatures
high pressures, high temperatures
high pressure, low...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases can be described using the van der Waals equation [P+(nʼa/V2)](V-nb) = nRT The values of a and b are given below for the two real gases oxygen and methane. The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the smallest is The gas that would be expected to behave most like an ideal gas at high pressures...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases can be described using the van der Waals equation [P+(ma/V2](V-nb) = nRT The values of a and bare given below for the two real gases xenon and argon The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the largest is The gas that would be expected to behave least like an ideal gas at high pressures is...
At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 23.0 g...
At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 23.0 g H2 at 20.0°C in a 1.00 L container assuming in Part 1 non-ideal behavior and in Part 2 ideal behavior. Use the van der Waals equation and data in the hint to calculate the pressure exerted. Now, calculate the pressure exerted, assuming that the gas behaves as an ideal gas.
At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 19.5 g...
At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 19.5 g H2 at 20.0°C in a 1.00 L container assuming in Part 1 non-ideal behavior and in Part 2 ideal behavior. 1.Use the van der Waals equation and data in the hint to calculate the pressure exerted. 2.Now, calculate the pressure exerted, assuming that the gas behaves as an ideal gas.
At high pressures, real gases do not behave ideally. (a) Use the van der Waals equation...
At high pressures, real gases do not behave ideally. (a) Use the van der Waals equation and data in the text to calculate the pressure exerted by 28.5 g H2 at 20 degree C in a 1.00 L container. Repeat the calculation assuming that the gas behaves like an ideal gas
9:08 LTE Question 22 of 23 Submit Under what conditions are gases most likely to behave...
9:08 LTE Question 22 of 23 Submit Under what conditions are gases most likely to behave ideally? A) High pressures B) Low temperatures C) Polar molecules D) Low pressures E) Large molecules Tap here or pull up for additional resources
Part A) Which of the following statements is true for ideal gases, but is not always...
Part A) Which of the following statements is true for ideal gases, but is not always true for real gases? Choose all that apply. Molecules are in constant random motion. Pressure is caused by molecule-wall collisions. The size of the molecules is unimportant compared to the distances between them. The volume occupied by the molecules is negligible compared to the volume of the container. Part B) Which of the following statements is true for real gases? Choose all that apply....
which gas would behave more ideally at the same condition of P and T? CO or...
which gas would behave more ideally at the same condition of P and T? CO or N2 Can you please show the equation?
Part 1: Which of the following gas samples would be most likely to behave ideally under...
Part 1: Which of the following gas samples would be most likely to behave ideally under the stated conditions? Explain. A) N2 at 1 atm and -70°C B) CO at 200 atm and 25°C C) SO2 at 2 atm and 50 °C D) Ne at STP E) NH3 at 1 atm and 25°C PART 2: Given that Na(l) + ½ O2 (g) ⇌ NaO (g) K1 = 2 x 105 Na2O2(s) + Na(l) ⇌ NaO(g) + Na2O(s) K2 =...
Show that low pressure chemical vapour deposition [low pressure combined with high gas velocity d...
Show that low pressure chemical vapour deposition [low pressure combined with high gas velocity due to pumping] results in surface reaction limited growth.
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases can be described using the van der Waals equation [P+(nʼa/V2)](V-nb) = nRT The values of a and b are given below for the two real gases oxygen and methane. The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the smallest is The gas that would be expected to behave most like an ideal gas at high pressures...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases can be described using the van der Waals equation [P+(ma/V2](V-nb) = nRT The values of a and bare given below for the two real gases xenon and argon The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the largest is The gas that would be expected to behave least like an ideal gas at high pressures is...
At high pressures, real gases do not behave ideally. (a) Use the van der Waals equation and data in the text to calculate the pressure exerted by 28.5 g H2 at 20 degree C in a 1.00 L container. Repeat the calculation assuming that the gas behaves like an ideal gas
9:08 LTE Question 22 of 23 Submit Under what conditions are gases most likely to behave ideally? A) High pressures B) Low temperatures C) Polar molecules D) Low pressures E) Large molecules Tap here or pull up for additional resources
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