using dehoff equation problem 1
Project Description:
1 use a dehoff equation and the thermodynamic table on d2l to establish a numerical equation giving the molar entropy of liquid water as a function of temperature at p=1 atm. do the same for water vapor. (assume cp is independent of temperature).
2 use these equations to calculate the entropy of vaporization of water at p=1 atm.
3 use the previous result to calculate the enthalpy of vaporization of water at p=1 atm.
4 from the enthalpy of vaporization of water calculate the total heat transfer qwater when 2 moles of water vapor at 100°c and 1 atm are cooled down to 50°c at at p=1 atm.
5 a block of copper of mass 2.00 kg and specific heat capacity cp=0.385 j/k·g at a temperature of 0°c is introduced in an insulated container in which there is 1 mole of water vapor at 100°c and 1 atm. what is the final temperature of the system at equilibrium assuming no heat transfer to the surrounding?
6 calculate the change in entropy δst for the total system during this process.
2 use these equations to calculate the entropy of vaporization of water at p=1 atm.
3 use the previous result to calculate the enthalpy of vaporization of water at p=1 atm.
4 from the enthalpy of vaporization of water calculate the total heat transfer qwater when 2 moles of water vapor at 100°c and 1 atm are cooled down to 50°c at at p=1 atm.
5 a block of copper of mass 2.00 kg and specific heat capacity cp=0.385 j/k·g at a temperature of 0°c is introduced in an insulated container in which there is 1 mole of water vapor at 100°c and 1 atm. what is the final temperature of the system at equilibrium assuming no heat transfer to the surrounding?
6 calculate the change in entropy δst for the total system during this process.
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