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l Lie vai der Waals constants. 5. Compare th e pressures given by the perfect gas...
Van der Waals Constants Gas CH4 CO2 Cl2 NH3 H20 Xe CCIA 02 N2 Kr a...
Van der Waals Constants Gas CH4 CO2 Cl2 NH3 H20 Xe CCIA 02 N2 Kr a b (bar.L2/mol2) (atm-L2/mol)(L/mol) 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 5.465 0.0305 4.192 4.137 0.0516 20.01 19.75 0.1281 1.382 1.363 1.370 1.351 5.121 5.193 1.355 0.0319 0.0387 0.0106 0.0320 0.0395 Ar 1.336 CO 1.472 1.452 4.544 4.481 0.0434 1.370 1.351 0.0387 3.852 3.799 0.0444 5.36 5.29 0.0443 H2S NO N20 NO2 SO2 HF HCI HBr 6.865 6.770 0.0568...
2.2. The equation of state of a van der Waals gas is given as P+)(v-b) =...
2.2. The equation of state of a van der Waals gas is given as P+)(v-b) = RT, CHAPTER 2: Simple Thermodynamic Systems 47 where a, b, and R are constants. Calculate the following quantities: т, From parts (a) and (b) calculate (av/OT)p
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas c...
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas con- stant, and a (L- atm/mol-) and b (L/mol) are material constants. Determine the volume of 1.5 mol of nitrogen (a .39 L2 atm/mol2. b = 0.03913 L/mol) at temperature of 350 K and pressure of 70 atm.
The van der Waals equation...
14-5. Using Eqs. (14-14) and (14-17), calculate the van der Waals constants a and b for nitrogen. For u(r), assume a Lennard-Jones 6-12 potential with ε and σ given in Table 12-3. Compare the...
14-5. Using Eqs. (14-14) and (14-17), calculate the van der Waals constants a and b for nitrogen. For u(r), assume a Lennard-Jones 6-12 potential with ε and σ given in Table 12-3. Compare these calculated values to the experimentally determined values, a 1.39 x 106 cm atm/mole and b-39.1 cm/mole. Such poor agreement is quite typical, simply indi- cating the inadequacy of the van der Waals equation. 14-2 THE VAN DER WAALS EQUATION We start with Eq. (14-3), and take...
Van der Waals Constants Gas CH4 CO2 Cl2 NH3 H20 Xe CCIA 02 N2 Kr a b (bar.L2/mol2) (atm-L2/mol)(L/mol) 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 5.465 0.0305 4.192 4.137 0.0516 20.01 19.75 0.1281 1.382 1.363 1.370 1.351 5.121 5.193 1.355 0.0319 0.0387 0.0106 0.0320 0.0395 Ar 1.336 CO 1.472 1.452 4.544 4.481 0.0434 1.370 1.351 0.0387 3.852 3.799 0.0444 5.36 5.29 0.0443 H2S NO N20 NO2 SO2 HF HCI HBr 6.865 6.770 0.0568...
2.2. The equation of state of a van der Waals gas is given as P+)(v-b) = RT, CHAPTER 2: Simple Thermodynamic Systems 47 where a, b, and R are constants. Calculate the following quantities: т, From parts (a) and (b) calculate (av/OT)p
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas con- stant, and a (L- atm/mol-) and b (L/mol) are material constants. Determine the volume of 1.5 mol of nitrogen (a .39 L2 atm/mol2. b = 0.03913 L/mol) at temperature of 350 K and pressure of 70 atm.
The van der Waals equation...
14-5. Using Eqs. (14-14) and (14-17), calculate the van der Waals constants a and b for nitrogen. For u(r), assume a Lennard-Jones 6-12 potential with ε and σ given in Table 12-3. Compare these calculated values to the experimentally determined values, a 1.39 x 106 cm atm/mole and b-39.1 cm/mole. Such poor agreement is quite typical, simply indi- cating the inadequacy of the van der Waals equation. 14-2 THE VAN DER WAALS EQUATION We start with Eq. (14-3), and take...
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