At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 27.0 g...

At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 27.0 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.

Expert Solution

Thanking you

queen_honey_blossom answered 2 years ago

At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 33.0 g...

At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 33.0 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. Part 1)Use the van der Waals equation and data in the hint to calculate the pressure exerted= ____atm Part 2)Now, calculate the pressue excerted assuming that the gas behaves as an ideal gas.= _____ atm

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 29.0 g H2 at 20 degree C in a 1.00 L container. (b) Repeat the calculation assuming that the gas behaves like an Ideal gas.

The gases behave as ideal at low pressure, however, at high pressure they deviate from the...

The gases behave as ideal at low pressure, however, at high pressure they deviate from the ideal behavior. Compare the input power required(in kW)for compressing oxygen gas by first assuming ideal behavior then the real behavior. Take inlet state at 10 MPa, 14°C and the final state after compression is 15 MPa, 127°C. You can ignore the effect of gravity and motion of the system.Assume mass flow rate of the gas as 9 kg/min

Calculate the vapor pressure of water above a solution prepared by dissolving 27.0 g of glycerin...

Calculate the vapor pressure of water above a solution prepared by dissolving 27.0 g of glycerin (C3H8O3) in 135 g of water at 343 K. (The vapor pressure of water at 343 K is 233.7 torr.) Ph2o=? Calculate the mass of ethylene glycol (C2H6O2) that must be added to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressure by 9.00 torr at 35∘C. The vapor pressure of pure ethanol at 35∘C is 1.00×102 torr. m=?

Calculate the vapor pressure of a solution containing 27.0 g of glycerin (C3H8O3) in 119 mL...

Calculate the vapor pressure of a solution containing 27.0 g of glycerin (C3H8O3) in 119 mL of water at 30.0 ∘C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic) and use a density of 1.00 g/mL for the water.

23 mg of nitrogen gas, assumed to behave ideally, at a pressure of 88 torr and...

23 mg of nitrogen gas, assumed to behave ideally, at a pressure of 88 torr and at 22oC undergoes an adiabatic free expansion into a vacuum (Joule experiment) to a final pressure of 34 torr. a) Is the process reversible? Why or why not? b) What is the final temperature of the system? Why? [ answer should be 22oC] c) What is ∆S for the system?

Contrast ideal vs. nonideal/real gases, and explain why very high pressure and very low temperature gases...

Contrast ideal vs. nonideal/real gases, and explain why very high pressure and very low temperature gases behave nonideally. (6 points)

Calculate the pressure in cm H2O exerted in the closed end of an apparatus if the...

Calculate the pressure in cm H2O exerted in the closed end of an apparatus if the atmospheric pressure is 720.0 torr and the height of the water coloumn is 22.3cm.

for low pressure effusion of gases how do I calculate area of pinhole and pinhole diameter?...

for low pressure effusion of gases how do I calculate area of pinhole and pinhole diameter? ln(P/P0) = -Ct dP/P = - (A/V)(RT/2πM)1/2 dt = -C dt (volume= 285cm3, T= 298.15K) I got relaxation constant 0.01049 microns/second = C This is for N2 ( nitrogen) How do i solve A (pinhole are)?

For ethane, Pc = 48.2 atm and Tc = 305.4 K. Calculate the pressure exerted by...

For ethane, Pc = 48.2 atm and Tc = 305.4 K. Calculate the pressure exerted by 50.0 g of C2H6 in a 200-cm3 vessel at 37.5°C. (c) the Redlich–Kwong equation; (d) the virial equation, given that for ethane B = -179 cm3/mol and C = 10400 cm6/mol2 at 30°C, and B = -157 cm3/mol and C = 9650 cm6/mol2 at 50°C. (c) P = ? atm (d) P = ? atm

Question