Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use...


Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 L vessel. Van der Waals<br>constants can be found in the van der Waals constants table.<br>P =<br>atm<br>Use the ideal gas equation to calculate the pressure under the same conditions.<br>P =<br>atm<br>Under these conditions, would you expect HI or CCl, to deviate more from ideal behavior? Why?<br>CCl because it occupies a larger volume and it has smaller dispersion forces between molecules.<br>HI because it occupies a smaller volume and it has smaller dispersion forces between molecules.<br>HI because it occupies a larger volume and it has smaller dispersion forces between molecules.<br>CCI, because it occupies a larger volume and it has greater dispersion forces between molecules.<br>HI because it occupies a smaller volume and it has greater dispersion forces between molecules.<br>CCI, because it occupies a smaller volume and it has greater dispersion forces between molecules.<br>

Extracted text: Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm Under these conditions, would you expect HI or CCl, to deviate more from ideal behavior? Why? CCl because it occupies a larger volume and it has smaller dispersion forces between molecules. HI because it occupies a smaller volume and it has smaller dispersion forces between molecules. HI because it occupies a larger volume and it has smaller dispersion forces between molecules. CCI, because it occupies a larger volume and it has greater dispersion forces between molecules. HI because it occupies a smaller volume and it has greater dispersion forces between molecules. CCI, because it occupies a smaller volume and it has greater dispersion forces between molecules.
Van der Waals Constants<br>la<br>a<br>Gas<br>,? /mol ² )<br>b (L/mol)<br>(bar · L2 /mol2) (atm ·<br>2.273<br>L<br>CH4<br>CO2<br>Cl2<br>NH3<br>H2O<br>Xe<br>CC4<br>02<br>N2<br>2.303<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>Kr<br>Ar<br>CO<br>H2S<br>5.193<br>1.355<br>1.472<br>4.544<br>5.121<br>1.336<br>1.452<br>0.0106<br>0.0320<br>0.0395<br>0.0434<br>0.0387<br>4.481<br>NO<br>N20<br>NO2<br>SO2<br>1.370<br>1.351<br>3.852<br>3.799<br>0.0444<br>5.36<br>5.29<br>0.0443<br>6.865<br>6.770<br>0.0568<br>HF<br>HCI<br>HBr<br>9.565<br>3.700<br>4.500<br>6.309<br>9.431<br>3.648<br>4.437<br>6.221<br>0.0739<br>0.0406<br>0.0442<br>0.0530<br>HI<br>

Extracted text: Van der Waals Constants la a Gas ,? /mol ² ) b (L/mol) (bar · L2 /mol2) (atm · 2.273 L CH4 CO2 Cl2 NH3 H2O Xe CC4 02 N2 2.303 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 Kr Ar CO H2S 5.193 1.355 1.472 4.544 5.121 1.336 1.452 0.0106 0.0320 0.0395 0.0434 0.0387 4.481 NO N20 NO2 SO2 1.370 1.351 3.852 3.799 0.0444 5.36 5.29 0.0443 6.865 6.770 0.0568 HF HCI HBr 9.565 3.700 4.500 6.309 9.431 3.648 4.437 6.221 0.0739 0.0406 0.0442 0.0530 HI
Jun 11, 2022
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