Question

Calculate the change in entropy of the system when 15.0g of ice at -12.0C is converted to water vapor at 105C at a constant pressure of 1bar. The constant pressure molar heat capacity ofH2O (s) and H2O (l) is 75.291J/mol K and that of H2O (g) is 33.58 J/K mol

Answer #1

Calculate the change in the
entropy of 2.0 kg of water when it is converted from liquid to
vapor.
Heat of fusion for water is
334*10^3 (J/kg)
Boiling pint of water is 373.15 K
Heat of vaporization for water is 2256*10^3 (J/kg)

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...

Calculate the change in entropy (in J/K) when 38.7 g of nitrogen
gas is heated at a constant pressure of 1.50 atm from 22.9 ºC to
88.2 ºC. (The molar specific heats are Cv is 20.8 J/(mol-K) and Cp
is 29.1 J/(mol-K) .)

Calculate the change in entropy (in J/K) when 52.8 g of nitrogen
gas is heated at a constant pressure of 1.50 atm from 16.5 ºC to
62.8 ºC. (The molar specific heats are Cv is 20.8 J/(mol-K) and Cp
is 29.1 J/(mol-K) .)

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...

Part A) Calculate the enthalpy change, ΔH, for the
process in which 38.6 g of water is converted from liquid at 0.3 ∘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).
Part B) How many grams of ice at -24.6 ∘C can be completely
converted to liquid at 9.4 ∘C if the available heat for this
process is 4.04×103 kJ ?
For ice, use a specific heat...

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

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...

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

Calculate the enthalpy change, ΔH, for the process in which 46.8
g of water is converted from liquid at 0.7 ∘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).

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