Use the van der Waals equation of state to calculate the pressure of 3.50 mol of H, S at 493K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. 28.33 Р—...

Use the van der Waals equation of state to calculate the pressure of 3.50 mol of H, S at 493K in a 4.60 L vessel. Van der Waals<br>constants can be found in the van der Waals constants table.<br>28.33<br>Р—<br>atm<br>Incorrect<br>Use the ideal gas equation to calculate the pressure under the same conditions.<br>P =<br>30.79<br>atm<br>In a 15.50 L vessel, the pressure of 3.50 mol of H,S at 493 K is 9.14 atm when calculated using the ideal gas equation and<br>9.00 atm when calculated using the van der Waals equation of state.<br>Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the<br>4.60 L vessel compared to the 15.50 L vessel?<br>The molecular volume is a smaller part of the total volume of the 4.60L vessel.<br>The molecular volume is a larger part of the total volume of the 4.60 L vessel.<br>The attractive forces between molecules become less of a factor at the higher pressure in the 4.60L vessel.<br>The attractive forces between molecules become a greater factor at the higher pressure in the 4.60 L vessel.<br>

Extracted text: Use the van der Waals equation of state to calculate the pressure of 3.50 mol of H, S at 493K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. 28.33 Р— atm Incorrect Use the ideal gas equation to calculate the pressure under the same conditions. P = 30.79 atm In a 15.50 L vessel, the pressure of 3.50 mol of H,S at 493 K is 9.14 atm when calculated using the ideal gas equation and 9.00 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 4.60 L vessel compared to the 15.50 L vessel? The molecular volume is a smaller part of the total volume of the 4.60L vessel. The molecular volume is a larger part of the total volume of the 4.60 L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 4.60L vessel. The attractive forces between molecules become a greater factor at the higher pressure in the 4.60 L vessel.

Van der Waals Constants<br>a<br>a<br>Gas<br>b (L/mol)<br>(bar · L2 /mol 2) (atm · L2 /mol 2 )<br>CH4<br>CO2<br>Cl2<br>NH3<br>H20<br>Xe<br>CI4<br>02<br>N2<br>2.303<br>2.273<br>0.0431<br>3.658<br>3.610<br>0.0429<br>6.343<br>6.260<br>0.0542<br>4.225<br>4.170<br>0.0371<br>5.537<br>4.192<br>5.465<br>4.137<br>0.0305<br>0.0516<br>20.01<br>19.75<br>0.1281<br>1.382<br>1.363<br>0.0319<br>1.370<br>1.351<br>0.0387<br>5.121<br>1.336<br>1.452<br>4.481<br>1.351<br>3.799<br>Kr<br>5.193<br>1.355<br>1.472<br>4.544<br>0.0106<br>0.0320<br>0.0395<br>0.0434<br>Ar<br>CO<br>H2S<br>NO<br>N20<br>NO2<br>SO2<br>HF<br>HCl<br>HBr<br>1.370<br>0.0387<br>3.852<br>0.0444<br>5.36<br>5.29<br>0.0443<br>6.865<br>9.565<br>3.700<br>4.500<br>6.309<br>6.770<br>9.431<br>3.648<br>4.437<br>6.221<br>0.0568<br>0.0739<br>0.0406<br>0.0442<br>0.0530<br>HI<br>

Extracted text: Van der Waals Constants a a Gas b (L/mol) (bar · L2 /mol 2) (atm · L2 /mol 2 ) CH4 CO2 Cl2 NH3 H20 Xe CI4 02 N2 2.303 2.273 0.0431 3.658 3.610 0.0429 6.343 6.260 0.0542 4.225 4.170 0.0371 5.537 4.192 5.465 4.137 0.0305 0.0516 20.01 19.75 0.1281 1.382 1.363 0.0319 1.370 1.351 0.0387 5.121 1.336 1.452 4.481 1.351 3.799 Kr 5.193 1.355 1.472 4.544 0.0106 0.0320 0.0395 0.0434 Ar CO H2S NO N20 NO2 SO2 HF HCl HBr 1.370 0.0387 3.852 0.0444 5.36 5.29 0.0443 6.865 9.565 3.700 4.500 6.309 6.770 9.431 3.648 4.437 6.221 0.0568 0.0739 0.0406 0.0442 0.0530 HI

Jun 11, 2022

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Use the van der Waals equation of state to calculate the pressure of 3.50 mol of H, S at 493K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. 28.33 Р—...

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