Question

How much heat (in kJ) is required to convert 420. g of liquid
H_{2}O at 24.5°C into steam at 146°C? (Assume that the
specific heat of liquid water is 4.184 J/g·°C, the specific heat of
steam is 2.078 J/g·°C, and that both values are constant over the
given temperature ranges. The normal boiling point of
H_{2}O is 100.0°C.)

Answer #1

Heat required = **1120.73
kJ**

How much heat (in kJ) is required to convert 420. g of liquid
H2O at 24.9°C into steam at 145°C? (Assume that the specific heat
of liquid water is 4.184 J/g·°C, the specific heat of steam is
2.078 J/g·°C, and that both values are constant over the given
temperature ranges. The normal boiling point of H2O is
100.0°C.)

Calculate the amount of heat ( in kJ) required to convert 344.0
g of liquid water at 22.5 oC into steam at 145.0
°C. ( Heat of vaporization of water at its boiling
point = 40.7 kJ/mol., specific heats of water and steam are 4.184
J/g °C and 2.01 J/g °C,
respectively. )

part A How much heat energy, in
kilojoules, is required to convert 69.0 g of ice at −18.0 ∘C to
water at 25.0 ∘C ? Part B How long would it take
for 1.50 mol of water at 100.0 ∘C to be converted completely into
steam if heat were added at a constant rate of 22.0 J/s ?
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)):...

1.Calculate the amount of energy (in kJ) necessary to convert
377 g of liquid water from 0 degree C to water vapor at 167 degress
C. The molar heat of vaporization (Hvap) of
water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g
degrees C, and for steam is 1.99 J/g degrees C. (Assume that the
specific heat values do not change over the range of temperatures
in the problem.)
2.Which substance has the highest vapor pressure at...

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

How much heat is required to convert solid ice with a mass of
605 g at a temperature of -22.5 °C to liquid water at a temperature
of 65.0 °C? The specific heat of ice is cice = 2100
J/kgK, the specific heat of water is cwater = 4186.8
J/kgK, and the heat of fusion for water is Lf = 334
kJ/kg.
(in J)

How much heat is required to convert solid ice with a mass of
760 g at a temperature of -16.0 °C to liquid water at a temperature
of 76.5 °C? The specific heat of ice is cice = 2100
J/kgK, the specific heat of water is cwater = 4186.8
J/kgK, and the heat of fusion for water is Lf = 334
kJ/kg.

How much heat is required to convert solid ice with a mass of
870 g and at a temperature of -22.5 °C to liquid water at a
temperature of 79.0 °C? (The specific heat of ice is cice = 2100
J/kgK, the specific heat of water is cwater = 4186.8 J/kgK, and the
heat of fusion for water is: Lf = 334 kJ/kg.)

How much heat is required to convert 22.8 g of liquid benzene
(C6H6) at 58 ∘C to gaseous benzene at 100 ∘C? The boiling point of
benzene is 80.1 ∘C and Cm [C6H6(l)] = 136.0 J/(mol⋅∘C), and ΔHvap =
30.72 kJ/mol, Cm [C6H6(g)] = 82.4 J/(mol⋅∘C).

1. Calculate the amount of heat required to convert 1 g of
liquid water at 67°C to steam at 100°C. The specific heat of liquid
water is 4.18 J/g°C and the heat of vaporization is 40.7
kJ/mol.
2400 J
2.2 kJ
8.31 J
22.6 kJ
40.8 kJ
2. Which one of the following is true about surfactants?
they act to decrease surface tension
they form micelles on the surface of water
none of these
they are generally very small, highly...

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