Question

How much heat, in joules and in calories, must be removed from 3.61 mol of water to lower its temperature from 23.7 to 11.5°C? Include the sign in your answer.

joules

calories

Answer #1

**q = msT**

**mass of water = moles * molarmass**

**
= 3.61*18**

**
= 64.98 grams**

**q = - 64.98*4.184*(23.7-11.5)**

** = - 3316.89 J**

** = - 3.31689 KJ**

** = - 792.75 calories**

**= - 0.79275 Kcalories**

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?

How much heat must be removed from 100 g of water at 25.0°C to
change it into ice at -10.0°C? The specific heat of ice is 2090
J/kg · K, and the specific heat of water is 4186 J/kg · K. For
water LF = 334,000 J/kg and LV = 2.256 ×
106 J/kg.

1. What quantity of energy, in joules, must be removed from a
134-g sample of C2H4(g) that is
initially at 22.29°C to its condensation point (-103.77°C) and then
change the gas to a liquid at that temperature?
_______________ J
Useful Information:
The molecular weight
of C2H4 is 28.052
g/mol.
The boiling point
of C2H4 is
-103.77°C.
The heat capacity of C2H4(g) is
1.529 J/gK
The heat of vaporization of
C2H4 is 13.53 kJ/mol.

How much heat must be removed from 300 pounds of blanched
vegetables at 192 degrees F to freeze them to a temperature of 23
degrees F? (The vegetables have a 60% water content and the
specific heat of solid vegetables is 0.24 BTU/lb F).

How much heat must be removed from 200 pounds of blanched
vegetables at 192 degrees F to freeze them to a temperature of 23
degrees F? (The vegetables have a 60% water content and the
specific heat of solid vegetables is 0.24 BTU/lb F)

How much heat must be removed from 400 pounds of blanched
vegetables at 197 degrees F to freeze them to a temperature of 25
degrees F? (The vegetables have a 60% water content and the
specific heat of solid vegetables is 0.24 BTU/lb F)

How much heat must be removed to make ice at -10 degrees C from
2kg of water at 20 degrees C (The latent heat of fusion for water
is.25X10^5 J/kg. The specific heat of water is 4190 J/kg K and for
ice is 2090 J/kg K.)
a. 7.95 X10^5
b. 8.37 X10^5
c.8.75 X10^5
d. 2.09x10^5

The body must burn calories to warm the water from 0°C to a body
temperature of 37°C. Assume a dieter drinks 2.4 kg (i.e., 2.4 L) of
ice water every day. The specific heat of water is 4.186 ×
103 J/(kg⋅°C) (1) How much energy, in joules, does the
dieter’s body need to provide to warm the water over a full year.
Take 365 days in a year (2) One pound of fat supplies 3400 kcal
(Cal) to the body,...

An ice cube tray of negligible mass contains 0.290 kg of water
at 14.0 ∘C. Part A How much joules of heat must be removed to cool
the water to 0.00∘C and freeze it? Part B How much calories of heat
must be removed?Part C How much Btu of heat must be removed?

How many joules heat must be added to 2.0 kg of ice at a
temperature of -30 °C to bring it to room temperature 20 °C?
(Specific heat capacity of ice is 2100 J/kg °C).
(Specific heat capacity of water is 4186 J/kg °C).
(Latent heat of water-ice is 3.33x105 J/kg)
Group of answer choices
126.52 kJ
959.44 kJ
4293.44 kJ
668.78 kJ

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