How much heat is required to raise the temperature of
12.0
g
of water from
−
35

°C
to
175

°C?

heat:
kcal

Q = 1.68 Kcal

Explanation:

∴ m H2O = 12.0 g

∴ T1 = 35°C ≅ 308 K

∴ T2 = 175°C ≅ 448 K

∴ ΔT = T2 - T1 = 175 - 35 = 140 °C

∴ Cp H2O = 1 cal /g.°C

⇒ Q = (12.0 g)(1 cal/g°C)(140 °C)

⇒ Q = (1680 cal)*(Kcal/1000 cal)

⇒ Q = 1.68 Kcal

a small container that holds a source of energy a solar cell that captures light energy and converts it into electricity a voltaic cell that uses the oxidation of a fuel to produce electricity

explanation: