In: Chemistry

How much heat is required to convert 84.9 g of ice at -17.0 C to steam at 114 C?

Q = heat change for conversion of ice at -17 ^{o}C to
ice at 0 ^{o}C + heat change for conversion of ice at
0^{o}C to water at 0^{o}C + heat change for
conversion of water at 0^{o}C to water at 100 ^{o}C
+heat change for conversion of water at 100 ^{o}C to vapour
at 100 ^{o}C+ heat change for conversion of vapour at 100
^{o}C to vapour at 114 ^{o}C

Amount of heat absorbed , Q = mcdt + mL + mc'dt + mL' + mc"dt"

= m(cdt + L + c'dt' + L' + c"dt" )

Where

m = mass of ice = 84.9 g

c” = Specific heat of steam = 2.1 J/g degree C

c' = Specific heat of water = 4.186 J/g degree C

c = Specific heat of ice = 2.09 J/g degree C

L’ = Heat of Vaporization of water = 2260 J/g

L= Heat of fusion of ice = 334.9 J/g

dt’’ = 114-100 = 14^{o}C

dt' = 100 -0 =100 ^{o}C

dt = 0-(-17)=17 ^{o}C

Plug the values we get Q = m(cdt + L + c'dt '+ L' + c"dt" )

= 261.3x10^{3} J

= 261.3 kJ

How much heat is needed to convert 888 g of ice at -30°C to
steam at 136°C? (The specific heats of ice, steam, and liquid are
2.03 J/g · °C, 1.99 J/g · °C, and 4.18 J/g·°C, respectively. The
heat of fusion is 6.02 kJ/mol and heat of vaporization is 40.79
kJ/mol.)
________ kJ

How much heat is needed to convert 889 g of ice at -10°C to
steam at 136°C? (The specific heats of ice, steam, and liquid are
2.03 J/g·°C, 1.99 J/g·°C, and 4.18 J/g·°C, respectively. The heat
of fusion is 6.02 kJ/mol and heat of vaporization is 40.79 kJ/mol.)
kJ

How much heat Q is required to change 17.0 g of ice at − 6.00 ∘
C to 17.0 g of steam at 137 ∘ C ?

Thermochemistry
1. How much heat is required to convert 180g of ice at -40C to
steam at 120C?
2. Write the thermochemical equation for the decomposition of
one mole of methanol, CH3OH(l), into its elements in their stable
states at 25C and 1atm.

How much heat is required to convert solid ice with a mass of
750 g and at a temperature of -26.5 °C to liquid water at a
temperature of 72.0 °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.)

A.)
How much heat energy, in kilojoules, is required to convert 60.0 g
of ice at -18 degrees celcius to water at 25 degrees celcius?
B.) How long would it take for 1.50 mol of water at 100
degrees Celsius to be converted completely into steam if heat were
added at a constant rate of 24.0 J/s?

How much heat is required to convert solid ice with a mass of
605 g and at a temperature of -12.5 °C to liquid water at a
temperature of 55.5 °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.)

Calculate the amount of heat required to convert
155 g of ice at -10oC to steam at
110oC? (Hint:
Hfusion
= 80cal/g and Hvaporization =
540cal/g - show your work on the left, final answer on the
right)

Part A: How much heat energy, in kilojoules, is required to
convert 45.0 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 18.0 J/s ?

Part A. How much heat energy, in kilojoules, is required to
convert 61.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express
your answer to three significant figures and include the
appropriate units.
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 25.0 J/s ? Express your answer to three
significant figures and include the...

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