Sandra Cash completed a lab exercise on May 4, 2011 involving measuring the mass of nuts, Styrofoam cups, cups with water, and water alone, as well as recording the initial and final temperatures. The document includes tables for recording the measurements but all values are listed as "__32.5 C__". It also provides calculations for determining the specific heat capacity of iron and poses three questions relating to heat transfer and the effect of specific heat capacity.

1. Name: Sandra Cash
Student ID: 971382
Date: May 4, 2011
CHE1006 Lab Exercise Ten Results
Conservation of Energy
Mass of nuts (batch one), g __32.5 C__
Mass of nuts (batch two), g __32.5 C__
Total mass of nuts, g __32.5 C__
Mass of Styrofoam cup(s), g __32.5 C__
Mass of cups plus water, g __32.5 C__
Mass of water, g __32.5 C__
Initial temperature of water in cups, ˚C __32.5 C__
Temperature of boiling water, ˚C __32.5 C__
Temperature of nuts in boiling water, ˚C __32.5 C__
Final temperature of water in cups, ˚C __32.5 C__
Final temperature of nuts in water in cups, ˚C __32.5 C__
Calculated specific heat capacity of iron; show calculations using the asterisk or parentheses for
multiplication, plus sign for addition, etc.:
CHE1006 Concepts of Chemistry -1- Lab Exercise Ten

2. The final temperature of the water/gold would be lower than the final temperature of the
water/iron because gold's specific heat capacity is 0.0308 which is lower than iron's.The larger
the number for specific heat capacity means the more heat is needed to raise its temperature.
Questions
1. Some heat is inevitably lost during the procedure (i.e., not all of the thermal energy from
the nuts is actually transferred to the water). At what point during the procedure is it likely
that the most heat is lost?
The final temperature of the water/gold would be lower than the final temperature of the
water/iron because gold's specific heat capacity is 0.0308 which is lower than iron's.The
larger the number for specific heat capacity means the more heat is needed to raise its
temperature.
2. Identify three entities which are probably absorbing at least small amounts of heat away
from the water/iron mixture. (This is a completely different question than Question One.)
The final temperature of the water/gold would be lower than the final temperature of the
water/iron because gold's specific heat capacity is 0.0308 which is lower than iron's.The
larger the number for specific heat capacity means the more heat is needed to raise its
temperature.
3. Suppose that we had money to burn and had some nuts custom fabricated out of gold
instead of iron. If the exact same procedure were carried out (same mass of water, same
mass of gold in place of iron, etc.), would the final temperature of the water/gold be higher
or lower than the final temperature of the water/iron that you recorded? Explain in terms of
the specific heat capacity, referring to the table of values in the introduction to this
exercise.
The final temperature of the water/gold would be lower than the final temperature of the
water/iron because gold's specific heat capacity is 0.0308 which is lower than iron's.The
larger the number for specific heat capacity means the more heat is needed to raise its
temperature.

3. v.3:8/09
CHE1006 Concepts of Chemistry -3- Lab Exercise Ten