Question

Calculate the change in entropy of the surroundings when 1.0 mol
of water vaporizes as 100^{0}C. The heat of vaporization of
water is 40.6 kj/mol

Answer #1

What is the entropy change to the surroundings when a small,
decorative ice scuplture at a temperature of 0 degrees C and
weighing 456 g melts on a granite tabletop if the temperature of
the granite is 12 degrees C and the process occurs reversibly?
Assume the final temperature of the water is 0 degrees C. The heat
of fusion of ice is 6.01 kJ/mol.

Part A Calculate the change in entropy that occurs in the system
when 56.7 g of water vaporizes from a liquid to a gas at its
boiling point (100.0?C). ?H?vap = 40.7 kJ/mol Express your answer
to three significant figures.

If the temperature of the surroundings is -244.32 °C, calculate
the entropy change (in J/K) for the system (ΔSsys), surroundings
(ΔSsur) and universe (ΔSuniverse) when 40.4 g of liquid oxygen (O2)
freezes. Report your answers to two decimal places. Tfus(°C)
-218.79 Tvap(°C) -182.96 ΔH°fus (kJ/mol) 0.44 ΔH°vap (kJ/mol)
6.82

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

If the temperature of the surroundings is 5.45 °C, calculate the
entropy change (in J/K) for the system (ΔSsys),
surroundings (ΔSsur) and universe
(ΔSuniverse) when 33.6 g of gaseous diethyl ether
(C4H10O) condenses. Report your answers to
two decimal places.
Tfus(°C)
-116.30
Tvap(°C)
34.50
ΔH°fus (kJ/mol)
7.27
ΔH°vap (kJ/mol)
26.52
i need these :
1- ΔSsys =
2- ΔSsur =
3 -ΔSuniverse =

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)

The enthalpy of vaporization of methanol is 35.27 kJ/ mol at
64.1 oC. Determine the entropy change in the system for
the vaporization of 2.00 moles of methanol. What is the entropy
change in the surroundings (assume Tsurr = 25
oC.)

Find the change in entropy (in kJ K-1) for the condensation of
2.3 g of water (H2O; 18.0 g mol-1) at 100 Celcius, if the enthalpy
of vaporization of water is 40.65 kJ mol-1.

calculate the molar entropy change when (a) water and (b)
benzene are evaporated at their boiling points at a pressure of 1
atm. what are the entropy changes in (i) the system, (ii) the
surroundings, and (iii) the universe, in each case?

Using standard thermodynamic data at 298K, calculate the entropy
change for the surroundings when 1.53 moles of N2(g) react at
standard conditions.
Consider the reaction
N2(g) +
2O2(g)2NO2(g)
S°surroundings = ___ J/K

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