Answer:
45.2
Step-by-step explanation:
Explanation:
The idea here is that you need to use the mass of water, the heat added to the sample, and the specific heat of water to find the resulting change in temperature.
The equation that establishes a relationship between heat absorbed and change in temperature looks like this
q
=
m
⋅
c
⋅
Δ
T
, where
q
- heat absorbed
m
- the mass of the sample
c
- the specific heat of water, equal to
4.18
J
g
∘
C
Δ
T
- the change in temperature, defined as final temperature minus initial temperature
Plug in your values and solve for
Δ
T
- do not forget to convert the added heat from kilojoules to Joules
q
=
m
⋅
c
⋅
Δ
T
⇒
Δ
T
=
q
m
⋅
c
Δ
T
=
1.0
⋅
10
3
J
50.0
g
⋅
4.18
J
g
∘
C
=
4.785
∘
C
So, if the temperature of the water changed by
4.785
∘
C
, and its final temperature is now
50.0
∘
C
, it follows that its initial temperature was
Δ
T
=
T
f
−
T
i
⇒
T
i
=
T
f
−
Δ
T
T
i
=
50.0
∘
C
−
4.785
∘
C
=
45.2
∘
C
