a 200.5g sample of methane (CH4) gas has a volume of 25.0 L at 25.0C. Calculate the pressure using the ideal gas law. Calculate the corrected pressure using the Van der Waals equation
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a 200.5g sample of methane (CH4) gas has a volume of 25.0 L at 25.0C. Calculate...
A 200.5 g sample of methane (CH4) gas has a volume of 25.0 L at 25.0°C. Calculate the pressure using the ideal gas law. Calculate the corrected pressure using the Van der Waal's equation. (a - 2.25 atm*L2 *mol 2.b -0.0428 L'mol-1)
A 200.5 g sample of methane gas has a volume of 25 L at 25 degrees celcius. Calculate the pressure using the ideal gas law. Calculate the corrected pressure using the van der waal's equation (a=2.25 atm L2 mol-2; b= 0.0428 L*mol-1)
According to the ideal gas law, a 0.9530 mol sample of methane gas in a 1.223 L container at 267.0 K should exert a pressure of 17.07 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For CH4 gas, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol. ___ %
A 9.386 mol sample of methane gas is maintained in a 0.7854 L container at 302.4 K. What is the pressure in atm calculated using the van der Waals' equation for CH4 gas under these conditions? For CH4, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol.
A 9.083 mol sample of methane gas is maintained in a 0.8377 L container at 304.9 K. What is the pressure in atm calculated using the van der Waals' equation for CH4 gas under these conditions? For CH4, a = 2.253 L^2atm/mol^2 and b = 4.278 x 10^-2 L/mol.
A 1.55-mol sample of nitrogen gas is maintained in a 0.730-L container at 292 K. Calculate the pressure of the gas using both the ideal gas law and the van der Waals equation (van der Waals constants for N2 are a = 1.39 L2atm/mol2 and b = 3.91×10-2 L/mol). Pideal gas equation = ______ atm Pvan der Waals =_____ atm
Calculate the pressure exerted by 10.5 moles of neon gas in a volume of 5.65 L at 25 ° C using (a) the ideal gas equation and (b) the van der Waals equation. (For neon, a = 0.211 atm · L2/mol2 and b = 0.0171 L/mol.) (a) atm (b) atm
Use the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of neon at a pressure of 500.0 bar and a temperature of 355.0 K. (Hint: One way to solve the van der Waals equation for V is to use successive approximations. Use the ideal gas law to get a preliminary estimate for V ITS 500BAR use bar please not ATM
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.
need help on part B a Calculate the pressure exerted by 20.0 g of Co, in a 600 ml. vessel at 298 K using the ideal gas equation. Then, recalculate the pressure using the van der Waals equation. Assuming that the pressure calculated from the van der Waals equation is correct, what is the percent error in the answer when using the ideal gas equation? Van der Waals constants for CO2 are: a = 3.50 -, and b=0.0427 L/mol; R...