Textbook Problem

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A 237-g piece of molybdenum, initially at 100.0 °C, is dropped into 244 g of water at 10.0 °C. When the system comes to thermal equilibrium, the temperature is 15.3 °C. What is the specific heat capacity of molybdenum?

Interpretation Introduction

Interpretation:

At thermal equilibrium, the specific heat capacity for a given mass of molybdenum placed in a beaker containing water has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1k.Energy gained or lost can be calculated using the below equation.

  $\text{q=C×m×ΔT}$

Where,

  q= energy gained or lost for a given mass of substance (m),

  C =specific heat capacity

  $\text{ΔT}$= change in temperature

Explanation of Solution

Given,

Mass of Mo=$\text{237g}$

Mass of water=$\text{244g}$

Assume the sum of ${\text{q}}_{\text{Mo}}$ and ${\text{q}}_{\text{water}}$ $\text{=0}$

  ${\text{[C}}_{\text{water}}{\text{×M}}_{\text{water}}{\text{(T}}_{\text{final}}{\text{-T}}_{\text{initial}}{\text{)]+[C}}_{\text{Mo}}{\text{×M}}_{}$