how much heat energy is required to raise the temperature of 1 gm mass of water to 14.2c to 15.5c in cal
Answers
Answer:
First, the water must be heated to 100 degrees celcius and then the 100 degree water must be turned into steam.
Using the equation
Q
=
m
c
Δ
T
we can calculate the amount of energy for heating the water to 100 degrees.
Q
=energy input
m
=mass of the matter to heat
c
=specific heat capacity of the matter to heat
Δ
T
=the temperature change of the matter
We know
m=45 g
c=4187 Joules per kilogram- the specific heat capacity of water.
Δ
T
= 100-43=57, how many degrees we must increase the water by to make it boil and turn into steam.
Hence we find
Q
Q
=
(
0.045
)
×
(
4187
)
×
(
57
)
Q
=
10721
≈
10.7
k
J
Now we must turn the water into steam. This is done by increasing the potential energy of the water without changing its temperature using something called Specific latent heat of vaporisation of water- which is the energy amount required to convert a a unit mass of water into steam at constant temperature.
It is given by the equation
Q
=
m
L
Q
= energy input
m
=mass of the matter to vaporize
L
=the specific latent heat
According to Wikipedia the value of the latent heat of vaporisation of water is:
L
=
2264.705
kj/kg
Plugging it in to the equation:
Q
=
2264.705
×
0.045
≈
101.9
k
J
So the total energy change from both of these coverstion are:
101.9
+
10.7
≈
112.6
k
J
112.6
k
J
Answer:
kjghkkdkdkdksk
jsjskskshsjsks
Explanation:
ijekdkdkdjdidkdhdksjs
