Question

A drop of water with a mass of 0.48 g is vaporized at 100 ∘C and condenses on the surface of a 55-g block of aluminum that is initially at 25 ∘C. If the heat released during condensation goes only toward heating the metal, what is the final temperature in Celsius of the metal block? (The specific heat capacity of aluminum is 0.903 J/(g⋅∘C).)

Express the temperature in Celsius to two significant figures.

Calculate the amount of heat required to vaporize 84.8 g of water at its boiling point.

Express the heat in kilojoules to three significant figures.

How much heat is required to vaporize 33.8 g of water at 100 ∘C?

Express the heat in kilojoules to three significant figures.

Answer #1

A.)
calculate the heat change in kilocalories for condensation of 3.5
kg of steam at 100 Celsius.(Express your answer as a positive value
using two significant figures and include the appropriate units)
B.) calculate the heat change in kilojoules for condensation
of 185 g of steam at 100 Celsius.
(Express your answer as a positive value using three
significant figures and include the appropriate units)

A block of an alloy of mass 37.0 g and at a temperature of 15.51
°C is placed in a calorimeter containing 41.0 g of water at 81.93
°C. If the final temperature of the alloy and water is 39.77 °C,
calculate the specific heat (in J/g/K) of the metal. The specific
heat of water is 4.184 J/g/K. Express your answer to ***(((three
significant figures)) in scientific notation.

A block of an alloy of mass 25.0 g and at a temperature of 6.52
°C is placed in a calorimeter containing 35.0 g of dichlorobenzene
at 84.98 °C. If the final temperature of the alloy and
dichlorobenzene is 48.00 °C, calculate the specific heat (in J/g/K)
of the metal. The specific heat of dichlorobenzene is 1.13 J/g/K.
Express your answer to three significant figures in scientific
notation.

A block of an alloy of mass 36.0 g and at a temperature of
275.21 K is placed in a calorimeter containing 34.0 g of water at
366.25 K. If the final temperature of the alloy and water is 324.25
K, calculate the specific heat (in J/g/K) of the metal. The
specific heat of water is 4.184 J/g/K. Express your answer to three
significant figures in scientific notation.

A 100-gram metal block is initially heated to 100 degrees
Celsius. The copper block is then placed in 200-grams of water at
20 degrees Celsius. The block and the water are allowed to come to
thermal equilibrium and reach a temperature of 23.52 degrees
Celsius. a.) What is the change in temperature of the block and the
water? b.) If the specific heat of water is 4.184 J/g C, what is
the heat gained by the water? c.) What is...

12.57
Suppose that 0.87 g of water condenses on a 80.0 g block of iron
that is initially at 22 ∘C.
If the heat released during condensation goes only to warming
the iron block, what is the final temperature (in ∘C) of the iron
block? (Assume a constant enthalpy of vaporization for water of
44.0 kJ/mol.)

41 g g of steam at 100 ºC is mixed with 177 g g of ice at 0 ºC.
The latent heat of fusion of water is 33.5 × 104 J/kg, and the
specific heat of water is 4186 J/kg∙K, the latent heat of
vaporization of water is 22.6 × 105 J/kg. Part A Determine the
amount of heat absorbed by ice at 0 ºC to make water at 0 ºC.
Express your answer using three significant figures. Part B...

1. A 50-g sample of iron at 100oC is put into 75 g of
water at 0oC. What is the final temperature of the
mixture? (The specific heat of iron is 0.11 cal/g
Co.)
2. A machine part consists of 0.10 kg of iron and 0.16 kg of
copper. How much heat is added to the gear if the temperature
increases by 35oC? [Hint: Compute the heat required for
each metal and add the numbers. State your answer in joules.]...

A 2.76 g lead weight, initially at 10.7 ∘C, is submerged in 8.17
g of water at 52.6 ∘C in an insulated container.
What is the final temperature of both the weight and the water
at thermal equilibrium?
Express the temperature in Celsius to three significant
figures.

Part A A calorimeter contains 21.0 mL of water at 11.0 ∘C . When
1.60 g of X (a substance with a molar mass of 72.0 g/mol ) is
added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the
temperature of the solution increases to 26.0 ∘C . Calculate the
enthalpy change, ΔH, for this reaction per mole of X. Assume that
the specific heat of the resulting solution is equal to that of
water [4.18 J/(g⋅∘C)], that density of water...

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