Thank you!!! Consider an insulated vessel at a constant pressure of 1 atm contai

Question

Thank you!!!

Consider an insulated vessel at a constant pressure of 1 atm containing 2 5 moles of liquid water at a temperature of 15 degree C. Now suppose that 10 moles of ice at a temperature of -10 degree C are added to the vessel, and the system is allowed to come to thermal equilibrium. What is the final composition of the system (i.e., how many moles of ice and liquid water are present at equilibrium)? The thermodynamic constants for H20 are: Cp,H2O(s) = 36.2 J mol-1 K-1, Cp,H2O(l) = 75.3 J mol-1 K-1, Delta Hfusion(at 0 degree C) = 6.01 k] mol-1. [Hint: Think about the different heat transfer processes that take place as you add some ice cubes to a glass of water, and note that not all of the ice will melt in this case.]

Explanation / Answer

by applying conservation of energy we can simoly equate the energy released =energy absorbed by the ice cubes and if the amount of energy exceeds the amount of energy used to bring the temp of ice cubes to 0*C than we have to consider the fusion of ice also takes place ....and than the extra bit of energy is used up in bringing up the temp of the water which came from the ice melting until the thermal equillibrium is established bw the ice and water......

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