Question

Find ΔG for melting ice at 0°C and 100 atm. At this temperature
and pressure conditions, the densities of the ice and liquid water
are 0.9168 g/cm^{3} and 1.000 g/cm^{3} ,
respectively

Answer #1

100 g of water is 100/18 = 5.556 moles

H = n H_{fus}

H = 5.556 x 6.0 kJ/mol

H = 33.33 kJ

S^{o} =
(n x H_{fus})/T

S^{o} =
(5.556 x 6.0)/273

S^{o} =
0.122 kJ/K

G = H -
T S^{o}

G = 33.33kJ - 273 x 0.122 J/K

**G =
0kJ**

Gold has an equilibrium melting temperature of 1337 K at 1 atm
and an enthalpy of fusion of 12,550 J/mol. Find the pressure at
which the equilibrium melting temperature is 1400 K.
Using this answer, calculate the entropy change for melting 1 mol
of gold. The densities of solid gold and liquid gold are 19.3 g/mL
and 17.3 g/mL and are assumed to be approximately constant under
all conditions

If the temperature of 1 mL of air at 1 atm and 0 degrees C is
raised to 100 degrees C at the same pressure, the volume becomes
1.3671 mL. Calculate the value of absolute zero for a thermometer
using air, assuming that the pressure-volume porduct is linear with
absolute temperature even at 1 atm. Compare your result with the
ice point temperature in Table 2.3. Ice point temperature =
273.15K

Steam at 100°C is added to ice at 0°C.
(a) Find the amount of ice melted and the final temperature when
the mass of steam is 14 g and the mass of ice is 65 g.
(b) Repeat with steam of mass 4.0 g and ice of mass 65
g.

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

When 15.0 g of ice at 0°C is melted in 100 g of water at 20.0°C,
the final temperature is 9.5°C. Find the heat of fusion of ice,
based on this data.

The normal freezing point of water is 0.0 oC. At this temperature
the density of liquid water is 1.000 g/ml and the density of ice is
0.917 g /ml. The increase in enthalpy for the melting of ice at
this temperature is 6010 J/mol. What is the freezing point of water
at 200 atmospheres?

he normal freezing point of water is 0.0 degrees celsius. at
this temperature the density of liquid water is 1.000 g/mL and
density of ice is 0.917 g/mL. the increase in enthalpy for the
melting ice at this temperature is 6010 J/mol. What is the freezing
point of the water at 200 atms?

A 10.84 kg block of ice has a temperature of -22.5o C. The
pressure is one atmosphere. The block absorbs 5.113×106 J of heat.
What is the final temperature of the liquid water? (Give your
answer in oC, but enter only the numerical portion--oC is
implied)
Tries 0/10

In Part A, we saw that ΔG∘=−242.1 kJ for the
hydrogenation of acetylene under standard conditions (all pressures
equal to 1 atm and the common reference temperature 298 K). In Part
B, you will determine the ΔG for the reaction under a
given set of nonstandard conditions.
Part B
At 25 ∘C the reaction from Part A has a composition as shown in
the table below.
Substance
Pressure
(atm)
C2H2(g)
3.95
H2(g)
5.65
C2H6(g)
5.25×10−2
What is the free energy...

100 g of solid ice at 0 degree Celcius is added to 500 g of
liquid water at 90 degree celcius. What is the final temperature?
What initial water temperature is required so that 10 g of ice
remain once equilibrium has been reached?

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