Chapter 5, Problem 97IL

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# The value of ΔU for the decomposition of 7.647 g of ammonium nitrate can be measured in a bomb calorimeter. The reaction that occurs isNH4NO3(s) → N2O(g) + 2 H2O(g)The temperature of the calorimeter, which contains 415 g of water, increases from 18.90 °C to 20.72 °C. The heat capacity of the bomb is 155 J/K. What is the value of ΔU for this reaction, in kl/mol?

Interpretation Introduction

Interpretation:

The change in internal energy has to be calculated.

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 Î”T=1.82K

Specific heat capacity of water is 4.184â€‰J/gK

Heat capacity of calorimeter is 155â€‰J/K

Mass of the water is 415â€‰g

Using specific capacity of heat equation

â€‚Â q=CÃ—mÃ—Î”T, the values calculated.

Heat absorbed by the calorimeter =155J/Kâ€‰Ã—â€‰1.82K =282J

Heat absorbed by water = 415gâ€‰Ã—â€‰4.184J/gKâ€‰Ã—â€‰1.82K = 3160J

Total heat absorbed =282â€‰â€‰Jâ€‰+â€‰3160â€‰Jâ€‰

### 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