Circle the situation most likely to resemble an ideal gas and indicate why:
1. Ar at 1.5 atm and 400 K OR H2O at 1.5 atm and 400 K
2. Ar at 100 atm and 250 K OR at 200 atm and 250 K
3.Ar at 1.5 atm and 200 K OR Ar at 1.5 atm and 300K.
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Circle the situation most likely to resemble an ideal gas and indicate why: 1. Ar at...
200 moles of an ideal gas at 1 atm pressure and T=300K, compress adiabatically to 2 atm, go isochorically back to 1 atm, then isobarically back to the initial conditions, how much work is done by the gas?
Complete the table for an ideal gas. Reaction Pressure Volume n T 1 1.5 atm 1.5 L 0.100 moles [answer1] 2 780 torr 250 mL [answer2] 25°C 3 1.0 atm [answer3] 0.500 moles 300 K
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Make a PV diagram showing the following sequential processes: 2.00 moles of an ideal gas at 400K, 1.00 atm. 1. expand isothermally from 65.6 L to 131.3 L at 400 K. 2. cooled isobarically from 65.6 L, 200 K 3. heated isochorically from 200 K back to 400 K
Make one PV diagram showing the following sequential processes: 2.00 moles of an ideal gas at 400K, 1.00 atm. 1. expand isothermally from 65.6 L to 131.3 L at 400 K. 2. cooled isobarically from 65.6 L, 200 K 3. heated isochorically from 200 K back to 400 K.
1. A sample of an ideal gas has a volume of 2.26 L at 278 K and 1.10 atm. Calculate the pressure when the volume is 1.80 L and the temperature is 303 K. 2. The volume of a sample of hydrogen gas was decreased from 10.76 L to 4.05 L at constant temperature. If the final pressure exerted by the hydrogen gas sample was 8.39 atm, what pressure did the hydrogen gas exert before its volume was decreased? 3....
Hint: % difference = 100×(P ideal - Pvan der Waals) / P idealAccording to the ideal gas law, a 9.843 mol sample of argon gas in a 0.8425 L container at 502.0 K should exert a pressure of 481.3 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Ar gas, a =1.345L2 atm/mol2 and b = 3.219×10-2 L/mol.
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