(1) Using the data found in BOB, calculate the pressure exerted by 2.500 moles of carbon...
Be sure to answer all parts. Calculate the pressure exerted by 2.65 moles of CO2 confined in a volume of 4.03 L at 456 K. What pressure is predicted by the ideal gas equation? The van der Waals constants for CQ area 3.59 atm. L2/mol2 and b 0.0427 L/mol. van der Waals equation: ideal gas equation: [24.6 ]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
calculate the pressure exerted by 2.50 moles of CO2 confined in a volume of 5.00 L at 450K. Compare the pressure with that predicted by the ideal gas equation.
Calculate the pressure exerted by 18.0 g of N2 in a 700. 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 N2 are: a= 1.39 atm*L^2/mol^2 , and b=0.0391 L/mol ; R=0.082057 L*atm/K*mol. Pideal gas law =...
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...
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 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.
Use the van der Waals equation of state to calculate the pressure of 3.70 mol of CCI4 at 499K in a 3.70 L vessel. Van der Waals constants can be found in the van der Waals constants table. Use the ideal gas equation to calculate the pressure under the same conditions. In a 15.00 L vessel, the pressure of 3.70 mol of CCI4 at 499 K is 10.1 atm when calculated using the ideal gas equation and 9.2 atm when calculated using...
Use the van der Waals equation of state to calculate the pressure of 2.40 mol of H2S at 499K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. Use the ideal gas equation to calculate the pressure under the same conditions. In a 16.30 L vessel, the pressure of 2.40 mol of H2S at 499 K is 6.03 atm when calculated using the ideal gas equation and 5.97 atm when calculated using the...
Use the van der Waals equation of state to calculate the pressure of 2.10 mol of Kr at 471 K in a 3.70L vessel. Van der Waals constants can be found in this table. Number P- 2.004 atm Use the ideal gas equation to calculate the pressure under the same conditions. Number P= 21.947 atm In a 15.5 L vessel, the pressure of 2.10 mol of Kr at 471 K is 5.24 atm when calculated using the ideal gas equation...