The enthalpy of fusion for water is 6.01 kJ/mol. Calculate the entropy change for 1.0 mole of ice melting to form liquid at 273 K

calculate the volume of 87% dry steam at 1200 kpa ?.

In a gas turbine plant, 1000 ° C from the combustion chamber and 1 MPa gases entering with pressure, the turbine with an isentropic efficiency of 90% expands up to pressure. Turbine well it is not insulated and the temperature of 25 ° C and 100 from the turbine during expansion It was determined that there is a significant heat loss to the environment at kPa pressure. has been. Characteristics of air for combustion products and the following using admissions; (a) The actual and reversible specific power output of the turbine, (b) Specific exergy of the air in the inlet and outlet conditions, (c) Second law efficiency, (d) Heat transfer between the turbine and its surroundings and the work produced by the turbine Exergy transfer amounts with, (e) Calculate the irreversibility of the whole process. Assumptions: (i) The power generated by the heat transfer from the turbine to its surroundings is 18% (ii) Consider variable specific heat

Using Clapeyron relationship, the enthalpy of evaporation of H₂O at 200°C is (than) the data provided in saturation table. equal to lower higher

Helium gas expands from 125 kPa , 350K, 0.25m^3 to 100kPa in a polytropic process with n = 1.667. Is the work positive, negative or zero? %3D

Explain two concept zero and -5kJ/K in the answer

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Calculate the entropy change in the melting of 1 kg of ice at 0 °C. Heat of fusion of ice = 334.72 J g-1.

What is the enthalpy change upon transforming 2 moles of Ti(hex) from 298K into Ti(bcc) at 1600K? • What is the entropy change upon transforming 2 moles of Ti(hex) from 298K into Ti(bcc) at 1600K? • What is the absolute entropy of 1 mole of Ti(bcc) at 1600K? • What is the enthalpy change for transforming 1 mole of Ti(g) from 1600K into Ti(bcc) at 1200K? • Develop a general temperature-dependent enthalpy equation for Ti(bcc) which is valid for temperatures between 1155K and 1943K. This equation should be general with a form similar to: [HT(Ti,bcc) - H1155(Ti,bcc)] = A + B•T + C•T2 + D/T + E•T3 • What is the enthalpy of vaporization of 1 mole of Ti(bcc) to Ti(g) at 1600K? • What is the entropy of vaporization of 1 mole of Ti(bcc) to Ti(g) at 1600K? • What is the enthalpy of vaporization of 1 mole of Ti(hex) to Ti(g) at 298K? • What is the entropy of vaporization of 1 mole of Ti(hex) to Ti(g) at 298K?