   Chapter 5, Problem 16PS

Chapter
Section
Textbook Problem

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.

q=C×m×ΔT

Where,

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

C =specific heat capacity

ΔT= change in temperature

Explanation

Given,

Mass of Mo=237g

Mass of water=244g

Assume the sum of qMo and qwater =0

[Cwater×Mwater(Tfinal-Tinitial)]+[CMo×M

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 