Question

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 .

Answer #1

Heat required for converting water to ice at 0°C,

= 1.10*333000 J

= 366300 J

Heat required for raising temperature of water from 0°C to 19°C,

= 1.10*4186*19

= 87487.4 J

Total heat required = 366300 + 87487.4 = 453787.4 J

Heat to be removed from steam at 100°C to convert into water at 100°C,

= 2260000*M

Heat to be removed to cool water at 100°C to water at 19°C

= M*4186*(100-19)

= 339066M

Total heat lost = (2260000 + 339066)*M = 2599066M

Total heat lost = total heat required

2599066*M = 453787.4

M = 453787.4/2599066

= 0.17 kg of steam

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=

Part A
What mass of steam at 100∘C must be added to 1.90 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∘ , the heat of
vaporization is 2260 kJ/kg .
Express your answer to two significant figures and include the
appropriate units.
m =

What mass of steam at 100°C must be mixed with 216 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 65.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg.

What mass of steam at 100°C must be mixed with 162 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 71.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg.

What mass of steam at 100°C must be mixed with 260 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 73.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg

What mass of steam at 100°C must be mixed with 301 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 16.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg.

100. g of ice at 0 degrees C is added to 300.0 g of water at 60
degrees C. Assuming no transfer of heat to the surroundings, what
is the temperature of the liquid water after all the ice has melted
and equilibrium is reached?
Specific Heat (ice)= 2.10 J/g C
Specific Heat (water)= 4.18 J/g C
Heat of fusion = 333 J/g
Heat of vaporization= 2258 J/g

45 gg of steam at 100 ºC is mixed with 177 gg 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.
a)Determine the amount of heat absorbed by ice at 0 ºC to make
water at 0 ºC.
b)Determine the amount of heat released by steam at 100 ºC to
make...

What mass of steam at 100 degrees C must be added to 2.15kg of
ice at 0 degrees C to yield liquid water at 30 degrees C?

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

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