BinyG12. How much heat (in kJ) must be added to 45.0 g of ice at -22.0°C to change it to water at 37.0°C?(Cice 4.10 J/g°C ; cwater 4.18 J/g°C; heat of fusion of ice/water 335 J/g.)

The following equation would be used

Answered: BinyG 12. How much heat (in kJ) must be…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter11: Liquids And Solids

Section: Chapter Questions

Problem 11.98QE

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Similar questions

Calculate the quantity of heating required to convert the water in four ice cubes (60.1 g each) from H2O(s) at 0 °C to H2O(g) at 100. °C. The enthalpy of fusion of ice is 333 J/g and the enthalpy of vaporization of liquid water is 2260 J/g.
Explain why 15 g of steam at 100C melts more ice than 15 g of liquid water at 100C.
The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.
The molar heat of fusion of sodium metal is 2.60 kJ/mol, whereas its heat of vaporization is 97.0 kJ/mol. a. Why is the heat of vaporization so much larger than the heat of fusion? b. What quantity of heat would be needed to melt 1.00 g sodium at its normal melting point? c. What quantity of heat would be needed to vaporize 1.00 g sodium at its normal boiling point? d. What quantity of heat would be evolved if 1.00 g sodium vapor condensed at its normal boiling point?
What phase changes will take place when water is subjected to varying pressure at a constant temperature of 0.005 C? At 40 C? At 40 C?
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.

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BinyG 12. How much heat (in kJ) must be added to 45.0 g of ice at -22.0°C to change it to water at 37.0°C? (Cice 4.10 J/g°C ; cwater 4.18 J/g°C; heat of fusion of ice/water 335 J/g.)