Worksheet 17
1
Worksheet #17
Calculating Heat
1. How much heat is needed to bring 12.0 g of water from 28.3 °C to 43.87 °C, if the
specific heat capacity of water is 4.184 J/(g•°C)?
2. How much heat is released when 143 g of ice is cooled from 14 °C to – 75 °C, if the
specific heat capacity of ice is 2.087 J/(g•°C).
3.
When 137 mL of water at 25 °C is mixed with 82 mL of water at 76 °C, what is the
final temperature of the water? Assume that no heat is lost to the surroundings and that
the density of water is 1.00 g/mL.
4. An unknown volume of water at 14.3 °C was added to 35.5 mL of water at 37.8 °C. If
the final temperature was 28.8 °C, what was the unknown volume? Assume that no heat
is lost to the surroundings and that the density of water is 1.00 g/mL
.
Determining Specific Heat Capacity
5.
An alloy of unknown composition is heated to 137 °C and placed into 100.0 g of
water at 25.0 °C. If the final temperature of the water was 36.4 °C, and the alloy
weighed 2.71 g, what is the specific heat capacity of the alloy? The specific heat of
water is 4.184 J/gºC.
6.
A 45.0 g rock is heated to 97.2 °C and placed into 75.3 g of water originally at 32.0
°C.
If the final temperature of the water was 46.2 °C, what is the specific heat
capacity of the rock?
7.
Given that the specific heat of gold is 0.129 J/gºC, calculate the final system
temperature if a 200.0 g block of gold at 100.0 ºC is placed in a coffeecup
calorimeter containing 50.0 g of water at an initial temperature of 25.0 ºC.
1.
How many calories are needed to raise the temperature of exactly 500 g of water
from 22.15 ºC to 24.70 ºC?
2.
How many joules are released when 30.0 mL of chloroform cool 18.0 ºC?
The s
pecific heat of chloroform is 0.971 J/(g)(ºC) and its density is 1.50 g/mL.
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 Fall '08
 Chemistry, Thermodynamics, Absolute Zero, Heat, °C, Thermodynamic temperature

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