Question

A) Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g
are combined with 140 g of water at 85 ∘Cin an insulated container.
(Δ*H*∘fus=6.02 kJ/mol, *c*water=4.18J/g⋅∘C)

If no heat is lost to the surroundings, what is the final temperature of the mixture?

B) A sample of steam with a mass of 0.510 g and at a temperature of 100 ∘C condenses into
an insulated container holding 4.50 g of water at 2.0 ∘C.(
Δ*H*∘vap=40.7 kJ/mol, *C*water=4.18
J/g⋅∘C)

Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?

Answer #1

A) Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g
are combined with 140 g of water at 85 ∘Cin an insulated container.
(Δ*H*∘fus=6.02 kJ/mol, *c*water=4.18J/g⋅∘C)

Hice + Hwater = 0

Hice = melting + cold water = mice*Latent heat + mice*Cwater*(Tf-0)

Hwater = hot water = mwater*Cwater*(Tf-85)

so

mice*Latent heat + mice*Cwater*(Tf-0) + mwater*Cwater*(Tf-85) = 0

53.5*334 + 53.5*4.184 * (Tf) + 140 * 4.184*(Tf-85) =

17869 + 53.5*4.184*Tf +585.76*(Tf-85) = 0

Tf(223.84 +585.76) = -17869 + 585.76*85

Tf = 31920.6 /(223.84 +585.76)

Tf = 39.42 °C

Four ice cubes at exactly 0 ∘C with a total mass of 55.0 g are
combined with 130 g of water at 80 ∘C in an insulated container.
(ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) If no heat is lost to the
surroundings, what is the final temperature of the mixture

Four ice cubes at exactly 0 ∘C with a total mass of 53.0 g are
combined with 140 g of water at 90 ∘C in an insulated container.
(ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C). If no heat is lost to the
surroundings, what is the final temperature of the mixture?

Four ice cubes at exactly 0 ∘C with a total mass of 51.5 g are
combined with 160 g of water at 75 ∘C in an insulated container.
(ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) . If no
heat is lost to the surroundings, what is the final temperature of
the mixture? Show Work

A sample of steam with a mass of 0.532 g at a temperature of 100
∘C condenses into an insulated container holding 4.25 g of water at
4.0 ∘C. (For water, ΔH∘vap=40.7 kJ/mol and
Cwater=4.18 J/(g⋅∘C).)
Assuming that no heat is lost to the surroundings, what is the
final temperature of the mixture?

A sample of steam with a mass of 0.520 g and at a temperature of
100 ∘C condenses into an insulated container holding 4.45 g of
water at 5.0 ∘C.( ΔH∘vap=40.7 kJ/mol, Cwater=4.18
J/g⋅∘C)
Assuming that no heat is lost to the surroundings, what is the
final temperature of the mixture?

1) A sample of steam with a mass of 0.505 g and at a temperature
of 100 ∘C condenses into an insulated container holding 4.25 g of
water at 3.0∘C.( ΔH∘vap=40.7 kJ/mol, Cwater=4.18
J/g⋅∘C)
Assuming that no heat is lost to the surroundings, what is the
final temperature of the mixture? In celcius!
2) Nanomaterials are materials that have dimensions on
the 1- to 100-nm scale. Carbon, metals, and semiconductors exhibit
distinct properties on the nanoscale that differ from their...

A sample of steam with a mass of 0.551 g and at a temperature of
100 ∘C condenses into an insulated container holding 4.20 g of
water at 5.0 ∘C . Assuming that no heat is lost to the
surroundings, what is the final temperature of the mixture? For
water, ΔHvap=40.7kJ/mol (at 100 ∘C)
. what is the temperate?

If the temperature of the surroundings is 38.36 °C, calculate
the entropy change (in J/K) for the system (ΔSsys), surroundings
(ΔSsur) and universe (ΔSuniverse) when 48.1 g of gaseous carbon
tetrachloride (CCl4) condenses. Report your answers to two decimal
places.
Tfus(°C) -23.00
Tvap(°C) 76.80
ΔH°fus (kJ/mol) 3.28
ΔH°vap (kJ/mol) 29.82

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

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