Question

A student places a 72.0 gram sample of metal at an initial temperature of 100.˚C in a coffee cup calorimeter that contains 40.0 grams of water at an initial temperature of 25.0 ˚C. After addition of the metal, the temperature of the water / metal mixture was monitored using a temperature probe. The highest temperature of the water / solid combination was found to be 35.0 ˚C. (The specific heat of water = 4.18 J / g ˚C )

Do not use spaces when giving your answers and remember significant figures

Useful equations: ΔT = Tfinal ̶ T initial ; q = specific heat × mass × ΔT

What was ΔT for the water? °C

What was ΔT for the metal? °C

How much heat ( q water ) did the water gain? J

Assuming no heat was lost to the surroundings, what is the value of q metal ? J

What is the specific heat of the metal? J / ( g °C )

Answer #1

Q = m c ∆T

Q = quantity of heat in joules (J)

m = mass of the substance acting as the environment in

grams (g)

c = specific heat capacity (4.19 for H2O) in J/(g
^{o}C)

∆T = change in temperature = Tfinal - Tinitial in ^{o}C

Heat was lost by metal = heat gained by water

Let us calculate heat gained by water

m = 40

c = 4.18

ΔT = 35-25 = 10

Q = 40 x 4.18 x 10 = 1672 Joules

**1672 joules of heat was gained by water . .**

specific heat of the metal

Q = 1672

m = 72 gm

C= ?

ΔT = 100 - 35 = 65

SUbstitute in the equation and find C

1672 = 72 x C x 65

C = 0.3573 J / ( g °C )

**.The specific heat of the metal is 0.3573 J / ( g °C
)**

A 72.5 gram piece of magnesium is heated to a temperature of
98.90ºC. The metal is then dropped into 40.0 grams of water at a
temperature of 18.50ºC inside a perfect calorimeter. Calculate the
final temperature of the water in the calorimeter. The specific
heat capacity for magnesium is Cp = 1.020 J/g·ºC.
Tfinal = ºC

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...

A calorimeter contains 82.4 grams of water at 20.9 °C. A 156
-gram piece of an unknown metal is heated to 81.9 °C and dropped
into the water. The entire system eventually reaches 26.6 °C.
Assuming all of the energy gained by the water comes from the
cooling of the metal—no energy loss to the calorimeter or the
surroundings—calculate the specific heat of the metal. The specific
heat of water is 4.18 J/g · °C _____J/g · °C

A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C)
is placed in a boiling water bath until the temperature of the
metal is 100.0*C. The metal is quickly transferred to 119.0g of
water at 25.0*C in a calorimeter (specific heat capacity of water =
4.18 J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is
placed in a boiling water bath until the temperature of the metal
is 100.0*C. The metal is quickly transferred to 119.0g of water at
25.0*C in a calorimeter (specific heat capacity of water = 4.18
J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

A 48.2 g sample of a metal is heated to 95.8 degrees C and
placed in a coffee-cup calorimeter containing 79.0 g of water at a
temperature of 18.5 degrees C. After the metal cools, the final
temperature of the metal and water is 22.8 degrees C. Calculate the
specific heat capacity of the metal, assuming that no heat escapes
to the surroundings or is transferred to the calorimeter.

3. A sample of metal weighing 35.5g at a temperature of 100 oC
was placed in a calorimeter containing 50 g of water at 25.0 oC. At
equilibrium the temperature of water and metal was 35.5 oC.
Calculate the heat capacity of the metal. . Use this value for
Cp:27.65.
4. When 0.50 g of magnesium metal is placed in a calorimeter,
and 100. mL of 1.0 M HCl were added the temperature of solution
increased from 22.2 oC to...

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...

Data
Balance temperature: 27ºC
Initial water temperature: 23ºC
Initial temperature of the metal part: 68ºC
Mass of the metal part: 193 grams
Mass of the empty calorimeter: 110 grams
Mass of the water inside the calorimeter: 250 grams
Specific heat of water: 4.19 J / gºC
Specific heat of the calorimeter (aluminum): 0.90 J / gºC
Experiment calculations
1- Calculate the heat gained by the water
2- Calculate the heat gained by the calorimeter
3- Calculate the specific heat of...

Calorimetry Problem: Show your work neatly and methodically.
Include the sign associated with ΔH.
1. When a 6.55 gram sample of solid sodium hydroxide dissolves
in 115.00 grams of water in a coffee-cup calorimeter, the
temperature rises from 21.6°C to 38.7°C. Calculate ΔH, in kJ/mole
NaOH, for the solution process. NaOH(s) Na1+(aq) + OH1- (aq) The
specific heat of the solution is 4.18 J/g °C. 3.
2, A 2.600 gram sample of phenol, C6H5OH, was burned in a bomb...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 43 seconds ago

asked 9 minutes ago

asked 9 minutes ago

asked 14 minutes ago

asked 14 minutes ago

asked 20 minutes ago

asked 48 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago