January 11, 2010. Learning Goal Clarify HW from this weekend Understand the concept of specific heat capacity In-Class Activities Semester 1 Review Quiz Pre-Lab Background Moodle Clarification HW Anything that did not get done this weekend! Specific Heat Capacity Pre-Lab
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Properties of Water
On a sunny day, the water in a swimming pool might only warm up a degree or two while the concrete around the pool may become too hot to walk on with your bare feet. This may seem strange because both the concrete and the water are being heated by the same source – The Sun. This evidence suggests it takes more heat to raise the temperature of some substances than others. This, in fact, is true: The amount of heat needed to raise the temperature of 1 gram of a substance by 1°C is called the specific heat capacity, or simply the specific heat, of that substance. Water has a specific heat value that is higher in comparison with the specific heats for other materials, such as concrete. In this lab, the specific heat of a metal will be used to calculate the specific heat of water.
The amount of heat needed to raise the temperature of 1 gram of a substance by 1°C is called the specific heat capacity, or simply the specific heat, of that substance.
Q = cpmΔT
#1) How much heat is absorbed when 50.0 grams of a substance cools from 25.0 ⁰C to 12.0 ⁰C? The specific heat of the substance is 1.2 J/g ⁰C.
cp = 1.2 J/g ⁰C
m = 50.0 grams
ΔT = 25.0 ⁰C - 12.0 ⁰C= 13.0 ⁰C
Q= (1.2 J/g ⁰C)(50.0 g)(13.0 ⁰C) = 780 Joules
#2) What is the specific heat (cp ) of a 25 gram object that absorbs 500 Joules of energy, which causes the temperature of the object to change from 12⁰C to 22⁰C?
Q = 500 J
ΔT = 22⁰C - 12⁰C = 10⁰C
m= 25 g
cp = 500 J /(25g)(10oC) = 2 J/g ⁰C