Question

Burns produced by steam at 100°C are much more severe than those produced by the same mass of 100°C water. To verify this, do the following.

(a) Calculate the heat (in kcal) that must be removed from 6.00 g of 100°C water to lower its temperature to 48.0°C.

(b) Calculate the heat (in kcal) that must be removed from 6.00 g of 100°C steam to condense it and lower its temperature to 48.0°C.

(c) Calculate (in kg) the mass of human flesh that the heat produced in each case can raise from the normal 37.0°C to 48.0°C. (Flesh is badly damaged at 50.0°C.)

Steam:______kg

Water: _______kg

Answer #1

The answer for above problem is explained below.

Burns produced by steam at 100°C are much more severe than those
produced by the same mass of 100°C water. To verify this:
(a) Calculate the heat that must be removed from 6.00 g of 100°C
water to lower its temperature to 45.0°C.
kcal
(b) Calculate the heat that must be removed from 6.00 g of 100°C
steam to condense it and lower its temperature to 45.0°C.
kcal
(c) Calculate the mass of human flesh that the heat produced in...

Why would burns caused by steam at 100◦C be more severe than
burns caused by (liquid) water at 100◦C, if the temperature is
initially the same in each case? (Hint: Consider the “useful
information” given below.)

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...

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).

A 50.0-g copper calorimeter contains 210 g of water at 20.0°C.
How much steam at 100°C must be condensed into the water if the
final temperature of the system is to reach 60.0°C?
A step-by-step process (ex. Q1+Q2+...+ Qn = 0) would be
appreciated. I am not concerned with the answer; I would just like
a clear setup of the problem.

A sample of steam with a mass of 0.532 g at a temperature of 100
∘C condenses into an insulated container holding 4.25 g of water at
4.0 ∘C. (For water, ΔH∘vap=40.7 kJ/mol and
Cwater=4.18 J/(g⋅∘C).)
Assuming that no heat is lost to the surroundings, what is the
final temperature of the mixture?

A coffee machine makes use of 100°C steam to warm up 0.18 kg
coffee at 14°C to 85°C. What is the mass of steam needed in g?
Assume that coffee has the same thermal properties as water, that
all heat from steam will be used to raise the temperature of the
coffee, and that steam used becomes part of coffee

A sample of steam with a mass of 0.551 g and at a temperature of
100 ∘C condenses into an insulated container holding 4.20 g of
water at 5.0 ∘C . Assuming that no heat is lost to the
surroundings, what is the final temperature of the mixture? For
water, ΔHvap=40.7kJ/mol (at 100 ∘C)
. what is the temperate?

8.33 kg of steam at temperature of 150 ∘C has 2.23×107 J of heat
removed from it. Determine the final temperature and phase of the
result once the heat has been removed if the heat is removed at
constant pressure during the gas phase. For this problem, use the
specific heat (at constant pressure) for water as 1850 J/kg∘C , the
latent heat of vaporization as 2.256×106 J/kg , the specific heat
of liquid water as 4186 J/kg∘C , the...

What mass of steam at 100°C must be mixed with 216 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 65.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg.

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