Question

Water has a heat of vaporization 40.7kJ/mole and a specific heat
of 4.18J/g o C.

How many joules of heat are required to boil a cup of tea? Assume
you start

with 250g of water at 25 o C and when the tea is complete you have
225g of

water at 100 o C (25g of water was boiled into steam at 100 o
C).

Answer #1

Using the values for the heat of fusion, specific heat of water,
and/or heat of vaporization, calculate the amount of heat energy in
each of the following:
A. joules needed to melt 90.0 g of ice at 0 ∘C and to warm the
liquid to 85.0
B. kilocalories released when 30.0 g of steam condenses at 100
∘C and the liquid cools to 0 ∘C
C. kilojoules needed to melt 26.0 g of ice at 0 ∘C, warm the
liquid...

The heat of fusion of water is 79.9 cal/g, the heat of
vaporization of water is 540 cal/g, and the specific heat of water
is 1.00 cal/deg/g. How many grams of ice at 0 ° could be converted
to steam at 100 °C by 9,076 cal of heat?

Using heat of fusion, specific heat of water, and/or heat of
vaporization, calculate the amount of heat energy in each of the
following.
(a) calories to condense 141 g of steam at 100

(a) How much energy does it take to heat 250 g of water from 20
◦C to the boiling point of 100 ◦C? (The specific heat of water is
4190 J/kg · K)
(b) (Suppose you wanted to cause the temperature change in part
(a) by using an 800W microwave. If we assume all the power
delivered by the microwave goes into the water, how long will it
take for the water to change temperature?
(c) The heat of vaporization...

Steam at 100.°C was passed into a flask containing 360.0 g of
water at 21°C where the steam condensed. How many grams of steam
must have condensed if the temperature of the water in the flask
was raised to 78°C? The heat of vaporization of water at 100.°C is
40.7 kJ/mol, and the specific heat is 4.18 J/(g·°C).

To change 25 kg of ice -10°C to steam 100°C, how much heat is
required? The specific heat of water is 4.184 kJ/kg. K. The latent
heat of fusion for water at 0°C is approximately 334 kJ/kg (or 80
cal/g), and the latent heat of vaporization at 100°C is about 2,230
kJ/kg (533 cal/g).

The water in your home has been temporarily shut off.
You want to boil some water for tea but all you have is a block of
ice (200 g) in your freezer. You put the ice in a pot and heat it
up. It takes 4 minutes to take the ice from (-10 degrees celsius)
to (100 degrees celsius). After 8 minutes how much water is left in
the pot?
The specific heat of ice is 2100 J/kg*C, the specific...

How much thermal energy (in J) is required to boil 2.25 kg of
water at 100.0°C into steam at 149.0°C? The latent heat of
vaporization of water is 2.26 ✕ 106 J/kg and the
specific heat of steam is
2010
J
kg · °C
.

2. Sixty grams of water is at an initial temperature of 24
°C.
Calculate the heat required to completely convert the 100 ºC
water to steam. (The latent heat of vaporization of water is 540
cal/g.)
The heat required to completely convert the 100 ºC water to
steam is... kcal?
3. How much heat is required to raise the temperature of 140 g
of water from 12°C to 88°C? The specific heat capacity of water is
1 cal/g·°C.
The heat...

Suppose the latent heat of vaporization of water is 540 cal/g.
how much heat (in calories) must be added to 50 grams of water at
an initial temperature of 20 C ( C represent degree Celsius) to a.
heat it to the boiling point?
b. then completely convert the water to steam?

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