Question

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

Answer #1

here the ice-water mixture remains at the end, so the final temperature of system = 0°C

Let the specific heat of the element be Cp

Heat released by element = 485.4 x Cp x (192 - 0)

= 93196.8 Cp J

Moles of ice melted = 117.0 / 18.02 = 6.493 mol

Heat absorbed by ice melting = 6.493 x 6.02 = 39086.57 J

Heat released = heat absorbed

93196.8 Cp = 39086.57

**Specific heat = 0.419
J/g°C**

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...

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

A 20.0-g sample of ice at 210.08C is mixed with 100.0 g water at
80.08C. Calculate the final temperature of the mixture assuming no
heat loss to the surroundings. The heat capacities of H 2 O(s) and
H 2 O(l) are 2.03 and 4.18 J/g ? 8C, respectively, and the enthalpy
of fusion for ice is 6.02 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

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

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.
(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?
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.(
ΔH∘vap=40.7 kJ/mol,...

There are 270 Calories in a Hershey's® Milk Chocolate
bar. The following data might be useful: ΔHvap
= 43.9 kJ/mol, ΔHfusion = 6.02 kJ/mol,
ΔHsublimation = 49.9 kJ/mol, specific heat of
ice = 2.05 J g-1°C-1, specific heat of water
= 4.18 J g-1°C-1, and specific heat of steam
= 2.08 J g-1°C-1. Assume the specific heat of
water does not change with temperature. (Density of ice = 0.920
g/mL).
How much energy is used up at each step of...

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

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, Tf, of the water
after all the ice melts.
Heat capactiy of H2o (s) = 37.7 J/(mol x K)
Heat capactiy of H2o (l) = 75.3
enthapy infusion of H20= 6.01 kj/mol

What quantity of energy does it take to convert 0.200 kg ice at
–20.°C to steam at 250.°C? Specific heat capacities: ice, 2.03
J/g·°C; liquid, 4.2 J/g·°C; steam, 2.0 J/g·°C; = 40.7
kJ/mol; = 6.02 kJ/mol.
What is the energy in kJ

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