A 920-g empty iron kettle is put on a stove. How much heat in joules must it absorb to raise its temperature form $15.0 ^ { \circ } \mathrm { C }$ to $93.0 ^ { \circ } \mathrm { C } \text { ? }$ The specific heat for iron is 113 cal/kg ∙ C°, and 1 cal = 4.186 J.

Question

Quizplus · Accepted Answer

The correct answer is A because the heat required to raise the temperature of the kettle is given by the formula Q = mcΔT, where m is the mass of the kettle, c is the specific heat of iron, and ΔT is the change in temperature. Plugging in the given values, we get Q = (0.920 kg)(113 cal/kg ∙ C°)(93.0 °C - 15.0 °C) = 33,900 J.

A 920-G Empty Iron Kettle Is Put on a Stove 15.0∘C15.0 ^ { \circ } \mathrm { C }15.0∘C

A 920-G Empty Iron Kettle Is Put on a Stove $15.0 ^ { \circ } \mathrm { C }$