Question

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 of the empty calorimeter is the heat capacity of the aluminum cup: 0.903 J g-1 oC-1. the density of water is: 1.00 g/mL. the heat capacity of water is: 4.184 J g-1 oC-1. Perform all calculations without rounding, but then provide your answer to the correct number of significant figures.

Part A

What is the change in heat, q, experienced by the cold water, in units of J?

Part B

What is the change in heat, q, experienced by the aluminum cup, in units of J?

Part C

What is the change in heat, q, experienced by the hot water, in units of J?

Part D

What is the change in heat, q, experienced by the metal object, in units of J?

Answer #1

The aluminum cup inside your calorimeter weighs 40.85 g. You add
49.81 g of water and 3.03 g of KCl to the calorimeter. The initial
temperature is 20.1oC, and the final temperature is 16.9oC. What is
the heat of dissolution for the amounts of salt added, in units of
J? Assume that: the calorimeter is completely insulated the heat
capacity of the empty calorimeter is the heat capacity of the
aluminum cup. the mass of KCl added is small enough...

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)

A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C .
A 124.0-g block of copper metal is heated to 100.4 ∘C by putting it
in a beaker of boiling water. The specific heat of Cu(s) is 0.385
J/g⋅K . The Cu is added to the calorimeter, and after a time the
contents of the cup reach a constant temperature of 30.3 ∘C .
Part A
Determine the amount of heat, in J , lost by the copper block....

A student wishes to determine the heat capacity of a coffee-cup
calorimeter. After she mixes 95.8 g of water at 62°C with 95.8 g of
water, already in the calorimeter, at 18.2°C, the final temperature
of the water is 35.0°C. Calculate the heat capacity of the
calorimeter in J/K. Use 4.184 J/g°C as the specific heat of
water.

When 10.0 g KOH is dissolved in 100.0 g of water in a coffee-cup
calorimeter, the temperature rises from 25.18 ˚C to 47.53 ˚C.
Calculate the ∆Hrxn for the dissolution process. Assume that the
solution has a specific heat capacity of 4.184 J/gK

An insulated aluminum calorimeter vessel of 150 g mass contains
300 g of liquid nitrogen boiling at 77 K. A metal block at an
initial temperature of 303 K is dropped into the liquid nitrogen.
It boils away 15.8 g of nitrogen in reaching thermal equilibrium.
The block is then withdrawn from the nitrogen and quickly
transferred to a second insulated copper calorimeter vessel of 200
g mass containing 500 g of water at 30.1 degrees celsius. The block
coolds...

You drop a 291-g silver figure of a polar bear into the 247-g
aluminum cup of a well-insulated calorimeter containing 261 g of
liquid water at 21.9°C. The bear\'s initial temperature is 97.9°C.
What is the final temperature of the water, cup, and bear when they
reach thermal equilibrium? The specific heats of silver, aluminum,
and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and
4190 J/(kg·K).

You drop a 297-g silver figure of a polar bear into the 247-g
aluminum cup of a well-insulated calorimeter containing 259 g of
liquid water at 22.3°C. The bear\'s initial temperature is 98.5°C.
What is the final temperature of the water, cup, and bear when they
reach thermal equilibrium? The specific heats of silver, aluminum,
and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and
4190 J/(kg·K).

You drop a 285-g silver figure of a polar bear into the 241-g
aluminum cup of a well-insulated calorimeter containing 263 g of
liquid water at 23.9°C. The bear\'s initial temperature is 95.9°C.
What is the final temperature of the water, cup, and bear when they
reach thermal equilibrium? The specific heats of silver, aluminum,
and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and
4190 J/(kg·K).

You drop a 297-g silver figure of a polar bear into the 205-g
aluminum cup of a well-insulated calorimeter containing 277 g of
liquid water at 24.5°C. The bear\'s initial temperature is 95.5°C.
What is the final temperature of the water, cup, and bear when they
reach thermal equilibrium? The specific heats of silver, aluminum,
and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and
4190 J/(kg·K).

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