Question

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.

Answer #1

What is the change in enthalpy (∆H) when a 147g of ice at
-23.7°C is heated to a liquid at 66.5°C? The specific heats of ice,
liquid water, and steam are 2.03, 4.18, and 1.84 J/g°C,
respectively. For water, ∆Hvap = 40.67 kJ/mol and ∆Hfus = 6.01
kJ/mol.

The
enthalpy change for converting 10.0g of ice at -50.0 degrees C to
water at 50.0 degrees C is ______ kJ. The specific heats of ice,
water, and steam are 2.09J/g-K, 4.18J/g-K, respectively. For H2O
Hfus=6.01kJ/mol and deltaHvap=40.67 kJ/mol.
A)12.28
B)4.38
C)3138
D)6.47
E)9.15

Calculate the amount of heat required to change 35.0g ice at
-25.0 C to steam at 125 C (Heat of fusion = 333 J/g; heat of
vaporization = 2260 J/g; Specific heats: ice = 2.09 J/g*K, water =
4.18 J/g*K, steam = 1.84 J/g*K)

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 –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

Please show each step. Thank you.
How much heat (in kJ) is evolved in converting 1.00 mole of
steam at 145.0 °C to ice at -50.0 °C? The heat capacity of ice is
2.09 J/g°C and that of steam is 2.09 J/g°C
Heat of fusion for water • Hfus = 6.02 kJ/mol
Heat of vaporization for water • Hvap = 40.7 kJ/mol

Calculate the enthalpy change, ΔH, for the process in
which 10.3 g of water is converted from liquid at 9.4 ∘C to vapor
at 25.0 ∘C .
For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and
Cs = 4.18 J/(g⋅∘C) for H2O(l).
How many grams of ice at -24.5 ∘C can be completely converted to
liquid at 9.8 ∘C if the available heat for this process is
5.03×103 kJ ?
For ice, use a specific heat of 2.01 J/(g⋅∘C) and...

Part A
Calculate the enthalpy change, ΔH, for the process in
which 44.0 g of water is converted from liquid at 7.6 ∘C to vapor
at 25.0 ∘C .
For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and
s = 4.18 J/(g⋅∘C) for H2O(l)
Express your answer numerically in kilojoules.
Part B
How many grams of ice at -11.0 ∘C can be completely converted to
liquid at 9.4 ∘C if the available heat for this process is
5.66×103 kJ...

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).

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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