Answer:
B. 0.302.
Explanation:
Q = m.c.ΔT,
where, Q is the amount of heat absorbed by water (Q = 0.954 J).
m is the mass of water (m = 0.755 g).
c is the specific heat capacity of water (c = 4.186 J/g.°C).
ΔT is the temperature difference (final T - initial T) (ΔT = ??? °C).
∴ ΔT = Q/m.c = (0.954 J)/(0.755 g)(4.186 J/g.°C) = 3.018 °C ≅ 3.02 °C.
Answer: Option (B) is the correct answer.
Explanation:
The given data is as follows.
mass = 0.755 g, Q = 0.954 J
[tex]\Delta T[/tex] = ? , Specific heat of water, C = [tex]4.18 J/g^{o}C[/tex]
As the relation between heat energy, mass and change in temperature are as follows.
Q = [tex]mC \Delta T[/tex]
0.954 J = [tex]0.755 g \times 4.18 J/g^{o}C \times \Delta T[/tex]
[tex]\Delta T = 0.302^{o}C[/tex]
Thus, we can conclude that increase in temperature is [tex]0.302^{o}C[/tex].
