Question

A iron cube with a mass of 25.0 grams was heated to 90 °C. Then dropped to a cup containing 100 grams of water at a temperature of 23.0 °C. After 10 minutes, the water and metal came to a temperature of 27 °C. Calculate the specific heat capacity of the metal?

Answer #1

A few iron nails with a total mass of 22.4 g are heated in a
water bath for five minutes. The water bath was boiling with a
constant temperature of 101°C according to the thermometer. When
the nails were carefully transferred into 182.0 g of water in a
coffee cup calorimeter the temperature of the water rose from
25.0°C to 26.0°C. What is the heat capacity of the iron?

A 35.7 gram sample of iron (heat capacity 0.45 g/J°C) was heated
to 99.10 °C and placed into a coffee cup calorimeter containing
42.92 grams of water initially at 15.15 °C. What will the final
temperature of the system be? (Specific heat of water is 4.184
J/g°C).
Please show 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)

An unknown metal of mass 0.280 kg is heated to 160.0°C and
dropped in an aluminum calorimeter of mass 0.250 kg that contains
0.170 kg of water at 30°C. The calorimeter, water, and unknown
metal have a final temperature of 46.0°C. Find the specific heat of
the unknown metal. Hint: you need the specific heat of water and
aluminum. Use units of [J/(kg.K)] and the values in your book for
the specific heat.

1. A 74.2-g piece of metal is heated to 89.55 degrees C and
dropped into 52.0 g of water at 23.22 degrees C in a calorimeter
with the heat capacity of 41.0 J/C . The
final temperature of the system is 27.60 degrees C.
a) Assuming that the metal does not react with water and
Cs(H2O) = 4.18 J/g*C , calculate
the specific heat capacity of the metal in
J/g*C
b) Most metals have the same molar heat capacity of...

A 25 g gold nugget with an initial temperature of 60 °C is
dropped into an insulated cup containing 100 ml of water initially
at a temperature of 5°C. What is the final temperature after
thermal equilibrium is established?
Table 3.4 Specific Heat Capacities of Some Common Substances
Substance Specific Heat Capacity (J/g °C) Lead 0.128 Gold 0.128
Silver 0.235 Copper 0.385 Iron 0.449 Aluminum 0.903 Ethanol 2.42
Water 4.184

A hot iron horseshoe ( mass = 0.40kg ) is dropped into 0.00135
m3 of water in a .930kg iron pot initially at 20.0 0C. If the final
equilibrium temperature is 25.0 0C. What was the initial
temperature of the hot horseshoe? ( specific heat of iron =
0.11kcal/kg 0C or 450J/kg 0C

A 306.4-milligram cube of iron is heated to 1,423°C and placed in a
calorimeter filled with77.1-mL of 25.0°C air. Calculate the
temperature at thermal equilibrium. The density of air is 1.225 x
10-3
g/cm3.

008
A 0.0456 kg ingot of metal is heated to 215◦C and then is
dropped into a beaker containing 0.415 kg of water initially at
19◦C. If the final equilibrium state of the mixed system is 21.4
◦C, find the specific heat of the metal. The specific heat of water
is 4186 J/kg · ◦ C.
Answer in units of J/kg · ◦ C.

A 46.5 g ice cube, initially at 0°C, is dropped into a Styrofoam
cup containing 348 g of water, initially at 21.4°C. What is the
final temperature of the water, if no heat is transferred to the
Styrofoam or the surroundings?

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