Question

The following information is given for ethanol at 1 atm:

Boiling Temp = 78.40°C

Delta H vaporization(78.40°C) = 837.0 J/g

Melting Temp = –114.50°C

Delta H fusion(–114.50°C) = 109.0 J/g

Specific heat gas = 1.430 J/g °C

Specific heat liquid = 2.460 J/g °C

A 45.30 g sample of liquid ethanol is initially at 19.90°C. If the sample is heated at constant pressure (P = 1 atm), ________ kJ of energy are needed to raise the temperature of the sample to 93.20°C.

Answer #1

Ti = 19.9

Tf = 93.2

here

Cl = 2.469 J/g.oC

Heat required to convert liquid from 19.9 oC to 78.4 oC

Q1 = m*Cl*(Tf-Ti)

= 45.3 g * 2.469 J/g.oC *(78.4-19.9) oC

= 6543 J

Lv = 837.0 J/g

Heat required to convert liquid to gas at 78.4 oC

Q2 = m*Lv

= 45.3g *837.0 J/g

= 37916 J

Cg = 1.43 J/g.oC

Heat required to convert vapour from 78.4 oC to 93.2 oC

Q3 = m*Cg*(Tf-Ti)

= 45.3 g * 1.43 J/g.oC *(93.2-78.4) oC

= 959 J

Total heat required = Q1 + Q2 + Q3

= 6543 J + 37916 J + 959 J

= 45418 J

= 45.4 KJ

Answer: 45.4 KJ

The following information is given for ether at 1 atm: boiling
point = 34.60°C Hvap(34.60°C) = 357.5 J/g melting point = -116.3°C
Hfus(-116.3°C) = 98.10 J/g specific heat gas = 1.460 J/g⋅°C
specific heat liquid = 2.320 J/g⋅°C A 27.70 g sample of liquid
ether is initially at -5.40°C. If the sample is heated at constant
pressure (P = 1 atm), __ kJ of energy are needed to raise the
temperature of the sample to 59.40°C.

The following information is given for cobalt at 1 atm: boiling
point = 3.097E3°C Hvap(3.097E3°C) = 6.603E3 J/g melting point =
1.495E3°C Hfus(1.495E3°C) = 262.7 J/g specific heat solid = 0.4180
J/g ⋅ °C specific heat liquid = 0.6860 J/g ⋅ °C A 38.00 g sample of
solid cobalt is initially at 1.467E3°C. If the sample is heated at
constant pressure (P = 1 atm), __ kJ of heat are needed to raise
the temperature of the sample to 1.963E3°C.

The following information is given for
n-pentane at 1 atm:
Tb =
36.20°C
Hvap(36.20°C) = J/g
Tm=
–129.70°C
Hfus(–129.70°C) = J/g
Specific heat gas =
1.650 J/g °C
Specific heat liquid =
2.280 J/g °C
A 47.80 g sample of liquid
n-pentane is initially at
–30.50°C. If the sample is heated at constant
pressure ( = 1 atm), kJ of energy are needed to raise
the temperature of the sample to 51.20°C.
______kJ

1) The following information is given for
n-pentane at 1 atm:
= 36.20°C
(36.20°C)
= J/g
=
–129.70°C
(–129.70°C)
= J/g
Specific heat gas =
1.650 J/g °C
Specific heat liquid =
2.280 J/g °C
A 40.00 g sample of liquid
n-pentane is initially at
–27.30°C. If the sample is heated at constant
pressure ( = 1 atm), _______kJ of energy are needed to raise the
temperature of the sample to 53.90°C.
2) The following information is given for
magnesium at 1...

The following information is given for bismuth
at 1 atm:
boiling point =
1.627E3 °C
Hvap(1.627E3°C) =
822.9 J/g
melting point =
271.0 °C
Hfus(271.0°C) = 52.60
J/g
specific heat solid=
0.1260 J/g ⋅ °C
specific heat liquid =
0.1510 J/g ⋅ °C
A 48.90 g sample of liquid
bismuth at 504.0 °C is poured
into a mold and allowed to cool to 24.0 °C. How
many kJ of energy are released in this process. Report the
answer as a...

How much heat energy is required to convert 21.1 g of solid
ethanol at -114.5 °C to gaseous ethanol at 191.5 °C? The molar heat
of fusion of ethanol is 4.60 kJ/mol and its molar heat of
vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of
-114.5 °C and a normal boiling point of 78.4 °C. The specific heat
capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous
ethanol is 1.43 J/g·°C.
________kJ

The following information is given for aluminum at 1 atm:
boiling point = 2.467E3 °C Hvap(2.467E3°C) = 1.053E4 J/g melting
point = 660.0 °C Hfus(660.0°C) = 398.4 J/g specific heat solid=
0.9000 J/g ⋅ °C specific heat liquid = 1.088 J/g ⋅ °C A 46.10 g
sample of liquid aluminum at 951.0 °C is poured into a mold and
allowed to cool to 28.0 °C. How many kJ of energy are released in
this process. Report the answer as a...

The following information is given for cadmium at 1atm:
boiling point = 765.0 °C Hvap(765.0 °C) = 889.6 J/g
melting point = 321.0 °C Hfus(321.0 °C) = 54.40 J/g
specific heat solid = 0.2300 J/g°C
specific heat liquid = 0.2640 J/g°C
A 20.60 g sample of liquid cadmium at 375.0 °C is poured into a
mold and allowed to cool to 28.0 °C. How many kJ of energy are
released in this process. Report the answer as a positive
number....

Using the following data,
Compound
Melting Point (C)
delta H fusion (kJ/mol)
Boiling Point (C)
delta H vap (kJ/mol)
HF
-83.11
4.577
19.54
25.18
HCl
-114.3
1.991
-84.9
17.53
HBr
-86.96
2.406
-67.0
19.27
Hl
-50.91
2.871
-35.38
21.16
calculate ?Sfus and ?Svap for HF.
Determine the entropy change when 3.30 mol of HF(g) condenses at
atmospheric pressure.

A substance has a melting point of 20°C and a heat of fusion of
2.6×104 J/kg. The boiling point is 150°C and the heat of
vaporization is 5.2×104 J/kg at a pressure of 1.0 atm. The specific
heats for the solid, liquid, and gaseous phases are 600 J/(kg·K),
1000 J/(kg·K), and 400 J/(kg·K), respectively. The quantity of heat
required to raise the temperature of 3.0 kg of the substance from
3°C to 118°C, at a pressure of 1.0 atm, is...

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