Question

In the laboratory, you are given a 18.5 g sample of an unknown
metal. The sample is irregular in shape, conducts heat and
electricity well, and sinks in water. The sample is placed into a
partially filled graduated cylinder and displaces 2.06 mL of water.
The sample is then heated to 160℃ with a Bunsen burner. The hot
metal is placed into a calorimeter filled with exactly 50.0 g of
water. The water temperature rises from 20℃ to 24.6℃ . Using the
above information and data table provided below, identify the metal
**and** explain your reasoning.

Metal | Density (g/cm^{3} ) |
Specific Heat (J/g*℃ ) |

A | 8.96 | 0.385 |

B | 8.96 | 0.233 |

C | 8.65 | 0.231 |

D | 7.31 | 0.385 |

Water | 1.00 | 4.184 |

Answer #1

here answer is almost equal to A here all the process is shown ...and i totally consider upto the 4 decimal .

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An irregular lump of an unknown metal has a measured density of
5.07 g/mL. The metal is heated to a temperature of 157 °C and
placed in a graduated cylinder filled with 25.0 mL of water at 25.0
°C. After the system has reached thermal equilibrium, the volume in
the cylinder is read at 30.5 mL, and the temperature is recorded as
45.5 °C. What is the specific heat of the unknown metal sample?
Assume no heat is lost to...

An irregular lump of an unknown metal has a measured density of
3.05 g/mL. The metal is heated to a temperature of 171 °C and
placed in a graduated cylinder filled with 25.0 mL of water at 25.0
°C. After the system has reached thermal equilibrium, the volume in
the cylinder is read at 34.3 mL, and the temperature is recorded as
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Assume no heat is lost to...

An irregular lump of an unknown metal has a measured density of
5.63 g/mL. The metal is heated to a temperature of 167 °C and
placed in a graduated cylinder filled with 25.0 mL of water at 25.0
°C. After the system has reached thermal equilibrium, the volume in
the cylinder is read at 31.9 mL, and the temperature is recorded as
39.5 °C. What is the specific heat of the unknown metal sample?
Assume no heat is lost to...

An irregular lump of an unknown metal has a measured density of
5.71 g/mL. The metal is heated to a temperature of 155 °C and
placed in a graduated cylinder filled with 25.0 mL of water at 25.0
°C. After the system has reached thermal equilibrium, the volume in
the cylinder is read at 32.9 mL, and the temperature is recorded as
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Assume no heat is lost to...

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.

You take a 150.485 g piece of copper
and
heat it over a
Bunsen burner. After a few
minutes of heating you place
the
heated
copper into 500 g of water at
25.00
̊C.
After
a
while you measure
the
temperature of
the water and find
that it is 45.32
̊C.
What was
the
temperature of the metal before
you put it in the water? The specific
heat of copper is
0.385
J/(g∙ ̊C).
Assume no energy was lost.

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.
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specific...

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A. Lead
B. Aluminum
C.Glass
D. Iron
E. Tin

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- How much heat (in J) did the metal give up to the water?
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calorimeter (3 significant figures).

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