Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: An open container holds ice of mass 0.570 kg at a temperature of -17.5°C. The mass of the container can be ignored. Heat is supplied to the container at the constant rate of 780 J/minute. The specific

Problem

An open container holds ice of mass 0.570 kg at a temperature of -17.5°C. The mass of the container can be ignored. Heat is supplied to the container at the constant rate of 780 J/minute. The specific heat of ice to is 2100 J/kg•K and the heat of fusion for ice is 334 x 103 J/kg.

How much time tmelts passes before the ice starts to melt?

From the time when the heating begins, how much time t  rise does it take before the temperature begins to rise above 0°C?

Solution

A) For the first question, we’re being asked to calculate the time it takes before the ice starts to melt.

So we have to calculate the amount of heat required to convert 0.570 kg of ice at -17.5 ˚C to 0.570 kg of ice at 0˚C

Then we have to get the time to reach that amount of heat based on the heat supplied (780 J/minute). 

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