The change of molar volume accompanying fusion of a solid organic compound is 0.55 cm³mol-1. Determine the change of chemical potential in units of kJ when pressure acting on the solid is increased from 7 to 4,200 bar.
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- 4.00 mol of perfect gas atoms with C p,m= 25 R is initially at 100.0 kPa, 100.0 dm3. It is heated to 150.0 dm3 at constant pressure and then heated to 150.0 kPa at constant volume. Calculate W, Q, ΔU and ΔH for this process.1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.Use the molar constant volume heat capacities for gases given in Topic 4C (as multiples for R) to estimate the change in reaction enthalpy of N2 (g) + 3 H2 (g) ---> 2 NH3 (g) when the temperture is increased from 300. K to 500. K. Ignore the vibrational contributions to heat capacity. Is the reaction more or less exothermic at the higher temperature? Atoms Linear Molecules Nonlinear Molecules Cv,m 3/2 R 5/2 R 3 R Cp,m 5/2 R 7/2 R 4 R
- A sample consisting of 0.10 mol of perfect gas molecules is held by a piston inside a cylinder such that the volume is 1.25 dm3; the external pressure is constant at 1.00 bar and the temperature is maintained at 300 K by a thermostat. The piston is released so that the gas can expand. Calculate (a) the volume of the gas when the expansion is complete; (b) the work done when the gas expands; (c) the heat absorbed by the system. Hence calculate ΔStot.The atomic heat capacity of solid Mo is given by the equation 0.503 x 105 Cp = 5.69 + 1.88 x 10-3 T – T² Find the change in entropy (in eu) which accompanies the heating of one mole of Mo from o C to its melting point, 2620°C. (Entropy unit, (eu) equal to i cal K-¹). Cp expression gives heat capacity in units of cal/mol.At 25 °C, the equilibrium partial pressures for the reaction A(g) + 2 B(g) 4 C(g)+D(g) were found to be PA = 4.45 bar, Pg = 5.82 bar, Pc = 5.74 bar, and Pp = 4.05 bar. %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 °C?
- At 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4 B(g)=2C(g)+D(g) were found to be PA = 4.74 bar, Pg 5.52 bar, Pc = 4.94 bar, and Pp 5.78 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ?4. The heat capacity of solid lead oxide is given by the equation: Cp(T) = 44.35 + 1.47 × 10-3 xT with T in units of K and the resulting Cp(T) in units of K-mol Calculate the change in enthalpy of 1 mole of PbO(s) if it is heated from 200 to 600 K at constant pressure. (Assume no phase transitions take place during this process.)(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol¹. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T +0.5 x 10³T ² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 10³T-² Cp(HCI)/JK ¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.
- A 1.65 mole sample of an ideal gas for which Cv, m = 3/2 R undergoes the following two-step process: (a) From an initial state of the gas described by T = 14.5 oC and P = 2x104 Pa, the gas undergoes isothermal expansion against a constant external pressure of 1.0x104 Pa until the volume has doubled. (b) Then the gas is cooled to constant volume. The temperature drops to -35.6 oC. Calculate q, w, ΔH, ΔU for each step and for the overall process.Calculate the change in internal energy (in kcal) for the reaction Cl2(g) + 7/2 O2(g) = Cl₂O7(g) at 25 °C, given that the gases are ideal. The enthalpy, AH, for the formation of Cl₂O7(g) is 63.4 kcal mol- ¹ at 25 °C.(a) An ideal gas of mass 4.5 g and molar mass of 17 g.mole-1 occupies 12.7 L at 310 K. Answer the following questions based on the conditions presented. (i) Calculate the work done under a constant external pressure of 30 kPa until the volume of gas has increased by 3.3 L. (ii) Calculate the work done in an isothermal and reversible expansion process resulting in a final volume of 16L. (iii) If the gas has a molar heat capacity of 30.8 J.mol-1.K-1 and is subjected to a constant volume process until it reaches a temperature of 350K, calculate the heat transfer in kJ.mol-1 of the gas. (b) Calculate the standard enthalpy of formation of N2O5 (g) from N2 (g) and O2 (g), in kJ. mol-1, from the following data: 2NO(g) + O2(g) ® 2NO2(g) DH = -114.1 kJ 4NO2(g) + O2(g) ® 2N2O5(g) DH = -110.2 kJ N2(g) + O2(g) ® 2NO(g) DH = +180.5 kJ