Question

A 1.000 kg block of ice at 0 °C is dropped into 1.354 kg of water that is 45 °C. What mass of ice melts?

Specific heat of ice = 2.092 J/(g*K) Water = 4.184 J/(g*K) Steam = 1.841 J/(g*K) Enthalpy of fusion = 6.008 kJ/mol Enthalpy of vaporization = 40.67 kJ/mol

Answer #1

How much heat is released when 105 g of steam at 100.0°C is
cooled to ice at -15.0°C? The enthalpy of vaporization of water is
40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the
molar heat capacity of liquid water is 75.4 J/(mol • °C), and the
molar heat capacity of ice is 36.4 J/(mol • °C).

To change 25 kg of ice -10°C to steam 100°C, how much heat is
required? The specific heat of water is 4.184 kJ/kg. K. The latent
heat of fusion for water at 0°C is approximately 334 kJ/kg (or 80
cal/g), and the latent heat of vaporization at 100°C is about 2,230
kJ/kg (533 cal/g).

What mass of steam at 100∘C must be added to 1.10 kg of ice at
0∘C to yield liquid water at 19 ∘C? The heat of fusion for water is
333 kJ/kg , the specific heat is 4186 J/kg⋅C∘ , the heat of
vaporization is 2260 kJ/kg .

What mass of steam at 100∘C must be added to 1.00 kg of ice at
0∘C to yield liquid water at 18 ∘C? The heat of fusion for water is
333 kJ/kg , the specific heat is 4186 J/kg⋅C∘J/kg⋅C∘ , the heat of
vaporization is 2260 kJ//kg .
Express your answer to two significant figures and include the
appropriate units
m=

A 500.0-g sample of an element at 153°C is dropped into an
ice-water mixture; 109.5-g of ice melts and an ice-water mixture
remains. Calculate the specific heat of the element from the
following data:
Specific heat capacity of ice: 2.03 J/g-°C
Specific heat capacity of water: 4.18 J/g-°C
H2O (s) → H2O (l), ΔHfusion: 6.02 kJ/mol (at 0°C)
a) If the molar heat capacity of the metal is 26.31 J/mol-°C,
what is the molar mass of the metal, and what...

The enthalpy change for converting 10.0 g of ice at -25.0
degrees C to water at 80.0 degrees C is _______kJ. The
specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K,
and 1.84 J/g-K, respectively. For H2O, Delta Hfus=6.01
kJ/mol, and Delta Hvap=40.67 Kj/mol
Please explain steps used as well. Thank you.

A 485.4-g sample of an element at 192°C is dropped into an
ice–water mixture; 117.0 g of ice melts and an ice–water mixture
remains. Calculate the specific heat of the element. ΔHfusion =
6.02 kJ/mol (for liquid water at 0°C). Specific heat =______
J/g∙°C

Two 20.0-g ice cubes at –20.0 °C are placed into 285 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, Tf, of the water
after all the ice melts. heat capacity of H2O(s) is 37.7 J/mol*K
heat capacity of H2O(l) is 75.3 J/mol*K enthalpy of fusion of H20
is 6.01 kJ/mol

Two 20.0-g ice cubes at –13.0 °C are placed into 275 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.
heat capacity of H2O(s)
37.7 J/(mol*k)
heat capacity of H2O(l)
75.3 J/(mol*k)
enthalpy of fusion of H2O
6.01 kJ/mol

Two 20.0-g ice cubes at –18.0 °C are placed into 245 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts. Please show work.
Heat capacity of H20(s): 37.7 J/(mol x K)
Heat capacity of H20(l): 75.3 J/(mol x K)
Enthalpy of fusion of H20: 6.01 kJ/mol

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