Question

a. An ice cold piece of aluminum metal is added to 50.0 g of hot water. Given the average initial temperature (76 C) calculated above for the hot water, calculate the heat, q, in joules of the piece of aluminum metal if the final temperature of the water is 40.0 °C. The specific heat of water is 4.184 J/g-°C. (0.50) b. Calculate the grams of aluminum metal used if the specific heat of aluminum is 0.895 J/g-°C. (0.50)

Answer #1

The aluminum cup inside your calorimeter weighs 39.96 g. You add
49.96 g of ice cold water to the calorimeter. You measure the
temperature of the calorimeter to be 0.5oC just before your next
addition. You then add 50.44 g of hot water and a 50.10 g metal
object, all having an initial temperature of 69.5oC. After the
calorimeter reaches thermal equilibrium, the final temperature is
measured to be 36.1oC. Assume that: the calorimeter is completely
insulated the heat capacity...

Calculate the specific heat of a metal from the following
experimental data. 75.0 ml cold water is taken in a calorimeter.
The initial temp of the water in the calorimeter is 21.2 degrees C.
To the calorimeter containing cold water 29.458 g metal at 98.9
degrees C is added. The final temperature of the contents of the
calorimeter is measured to be 29.5 degreesC. (Given: density of
water= 1.00 g/ml, specific heat of water= 4.184 J. G. -1 degrees C...

1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water
at 21.0°C contained in a calorimeter. The metal and water come to
the same temperature at 27.0°C.
- How much heat (in J) did the metal give up to the water?
(Assume the specific heat of water is 4.18 J/g·°C across the
temperature range.)
- What is the specific heat (in J/g·°C) of the metal?
2. A 0.529 g sample of KCl is added...

Suppose that 100.0 g of ice at 0 degrees Celsius are added to
300.0 g of water at 25.00 degrees Celsius. Is this sufficient ice
to lower the temperature of the water to 5.00 degrees Celsius and
still have ice remaining? Calculate the energy (heat), which must
be removed from water to achieve the desired temperature change,
and then prove that there is (is not) sufficient ice to cool the
water. Use the specific heat capacity of water (4.184 J/g-*C)...

An 100-g aluminum calorimeter contains 280 g of water at an
equilibrium temperature of 20°C. A 170-g piece of metal, initially
at 277°C, is added to the calorimeter. The final temperature at
equilibrium is 32°C. Assume there is no external heat exchange. The
specific heats of aluminum and water are 910 J/kg·K and 4190
J/kg·K, respectively. The specific heat of the metal is closest
to:
a) 270 J/kg·K.
b) 240 J/kg·K.
c) 330 J/kg·K.
d) 390 J/kg·K.
e) 360 J/kg·K.

A hot lump of 26.3 g of aluminum at an initial temperature of
67.2 °C is placed in 50.0 mL of H2O initially at 25.0 °C and
allowed to reach thermal equilibrium. What is the final temperature
of the aluminum and water given that the specific heat of aluminum
is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.

803 cal of heat is added to 5.00 g ice at –20.0 °C.
What is the final temperature of the water?
SPecific heat H2O(s)= 2.087 J/(g*C)
Specific heat H2O(l)=4.184 J/(g*C)
Heat of fusion= 333.6 J/g

A hot lump of 42.6 g of aluminum at an initial temperature of
62.2 °C is placed in 50.0 mL of H2O initially at 25.0 °C and
allowed to reach thermal equilibrium. What is the final temperature
of the aluminum and water given that the specific heat of aluminum
is 0.903 J/(g·°C)? Assume no heat is lost to surroundings. Please
show all work

A piece of titanium metal with a mass of 20.8 g is heated in
boiling water to 99.5 0C and then dropped into a coffee
cup calorimeter containing 75.0 g of water at 21.7
0C.When thermal equilibum is reached, the final
temperature is 14.30C.Calculate the specific heat
capacity of titanium. ( Specific Heat Capacity of H2O
(l) =4.184 J g-1 0C-1)

A metal sample weighing 72.1 g is placed in a hot water bath at
95.0 oC. The calorimeter contains 42.3 g of deoinized water. The
initial temperature of the water is 22.3 oC. The metal is
transferred to the calorimeter and the final temperature reached by
the water + metal is 32.2 oC.
A. Calculate ∆T for the water (Tfinal – Tinitial).
B. Calculate ∆T for the metal.
C. The specific heat of water is 4.18 J/goC. Calculate the
specific...

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