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

Consider the heating curve shown below for 22.86 grams of an unknown substance. You may assume constant pressure conditions. Note: the points are labeled as (amount of heat added, temperature). 

Given that the heat capacity at constant pressure for the liquid is 112.4 J/mol∙K, calculate how many moles of the compound are present in the sample being heated. Show all work and circle your final answer.


We are asked to calculate how many moles of the compound are present in the sample being heated given the heat capacity for the liquid and the heating diagram.

We go through the following steps to solve this problem:

Step 1. Calculate the amount of heat added based on the heating curve

Step 2. Calculate the mole of the substance

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