Calculate the amount of heat required to raise the temperature of a 65-g sample of water from 32 ∘c to 65 ∘c. (the specific heat capacity of water is 4.184 j/(g⋅∘c).

The amount of heat required is 9.0 kJ.

q = mCΔT

ΔT = T_f – T_i = 65 °C – 32 °C = 33 °C

q = 65 g × 4.184 J·°C⁻¹g⁻¹ × 33 °C = 9000 J = 9.0 kJ

8974.68 J.

Explanation:

Q = m.C.ΔT, where,

Q is the amount of heat required to raise the temperature of water sample,

m is the mass of water sample (m = 65.0 g),

C is the specific heat of water (C = 4.184 J/g.°C),

ΔT is the temperature difference (the final temperature - the initial temperature (ΔT = 65.0 - 32.0 = 33.0 °C).

∴ The amount of heat required to raise the temperature of water sample Q = m.C.ΔT = (65.0 g) (4.184 J/g.°C) (33.0 °C) = 8974.68 J.

it takes on an electronical energy