The normal boiling point of liquid benzene is 80.20 °C and its vapor pressure is 0.10 bar at 20.00°C. Calculate: (a) The value of AH vap m (b) The value of AS at the normal boiling point vap m
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- 1 at 1.00 atm and 154 °C, its melting temperature. The molar volume of the liquid at this e. (h) A certain solid occupies a container with volume 0.142 dm mol temperature and pressure is 0.1526 dm mol1 At 11.84 atm the melting temperature changes to 156° C. Calculate the enthalpy and entropy of fusion of the solid using the equation below (submit via link) dP AfusS dT AfusVDoes the entropy of the system increase, decrease, or staythe same when (a) a solid melts, (b) a gas liquefies, (c) asolid sublimes?Suppose that an infinitesimal crystal of ice is added to 10.0 g of supercooled liquid water at -10.0 °C in an adiatic container and the system reaches equilibrium at fixed pressure of 1 atm. a) What is AH for the process? b) The equibrium state will contain some ice and will therefore consist either of ice plus liquid at 0 °C or of ice below 0°C. Use the answer to (a) to deduce exactly what is present at equilibrium. c) Calculate AS for process.
- The AH,ap for water is 40.66 kJ mol- at the normal boiling point, T, = 373 K. Assuming AHap and ASap are approxi- mately independent of temperature from 50°C to 100°C, estimate the vapor pressure of water at 50°C (323 K).Consider the vaporization of liquid water to steam at apressure of 1 atm. (a) Is this process endothermic or exothermic?(b) In what temperature range is it a spontaneousprocess? (c) In what temperature range is it a nonspontaneousprocess? (d) At what temperature are the two phasesin equilibrium?The following gaseous system is in equilibrium at 30.00C and 1 bar, where 25% of N2O4 is dissociated into NO2: N2O4(g) 2 NO2(g) (a) Calculate the equilibrium constant, K. (b) Calculate the extent of the dissociation, a at 30.00C and 0.1 bar.
- If E°cell > 0, then what the value is of change in Gibbs free energy (G and the process is spontaneous?.7.2(a) Dinitrogen tetroxide is 18.46 per cent dissociated at 25°C and 1.00 bar in the equilibrium N2O4(g) 5 2 NO2(g). Calculate (a) K at 25°C, (b) ∆r G7 , (c) K at 100°C given that ∆r H7 = +57.2 kJ mol−1 over the temperature range.Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(9) +0,) M,0,(3) For this reaction, AH;= -5.268 kJ/mol and AS = 10.78 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AG= kJ/mol What is the equilibrium constant of this reaction at 298 K? Kp = What is the equilibrium pressure of O, (g) over M(s) at 298 K? atm Po,
- It is known that naphthalene, C10H8 melts at 80.2 0 If the vapor pressure of the liquid is 10 torr at 85.8 0C and 40 torr at 119.3oC, use the Clausius-Clapeyron equation to calculate: (a) The enthalpy of vaporization (b) The normal boiling point (c) The entropy of vaporization at the normal boiling point(iv) If E°cell > 0, then what the value is of change in Gibbs free energy AG and the process is spontaneous?.Many salts produce heat when dissolved in water andthe solution becomes warm, reflecting the fact that the Hterm is positive. In other cases the solution becomes quitecold and the enthalpy term is negative. What must be trueabout the Gibbs equation for these reactions to bespontaneous?