350.0 gram of ice at 0°C is placed in an insulated container at 20 °C and 1.0 L of water at 20°C was mixed with the ice. Calculate how many grams of ice would remain (if any) after water and ice reach to an equilibrium at 0°C. Assume that the heat capacity of the container is equal to that of 100.0 g of liquid water and the density of water is 1.000 g/mL. Heat of fusion of ice 6.01 kJ/mol and specific heat of water is 4.182 J/g°C.
350.0 gram of ice at 0°C is placed in an insulated container at 20 °C and 1.0 L of water at 20°C was mixed with the ice. Calculate how many grams of ice would remain (if any) after water and ice reach to an equilibrium at 0°C. Assume that the heat capacity of the container is equal to that of 100.0 g of liquid water and the density of water is 1.000 g/mL. Heat of fusion of ice 6.01 kJ/mol and specific heat of water is 4.182 J/g°C.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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350.0 gram of ice at 0°C is placed in an insulated container at 20 °C and 1.0 L of
water at 20°C was mixed with the ice. Calculate how many grams of ice would remain (if any)
after water and ice reach to an equilibrium at 0°C. Assume that the heat capacity of the
container is equal to that of 100.0 g of liquid water and the density of water is 1.000 g/mL.
Heat of fusion of ice 6.01 kJ/mol and specific heat of water is 4.182 J/g°C.
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