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A 15.7-g aluminum block is warmed to 53.2 °C and plunged

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 107P Chapter 3

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 107P

A 15.7-g aluminum block is warmed to 53.2 °C and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 °C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?

Step-by-Step Solution:

Solution 107P

Here. we are going to calculate the final temperature of the water and Al.

When two systems are combined together, then thermal energy is transferred from hotter body to cooler one. Thus, the heat absorbed by one system is equal to the heat released by another system

Therefore,

Qsystem (1) = - Q system(2) -----(1)

Step 1: 

Thermal energy transfer from metal to water.

From equation(1),

Qmetal = - Qwater

m metal x Cs metal x metal = -m water x Cs water x water -----(2)

Step 2:

Calculation of final temperature of water and Al metal.

Given,

Mass of Al metal, m metal = 15.7 g

Initial temperature of Al metal T1 = 53.2 °C

Mass of Water, m water = 32.5 g

Initial temperature of water T1 = 24.5 °C

Heat capacity,

Cs, H2O = 4.18 J/g oC ;

Cs,Al = 0.903J/g oC

From the equation (1)

m metal x Cs metal x metal = -m water x Cs water x water

 15.7 g x 0.903J/g oC x metal = - 32.5 g x4.18 J/g oC x  water

x metal = - 135.85 x water -------(2)

Step 3 of 3

Chapter 3, Problem 107P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The answer to “A 15.7-g aluminum block is warmed to 53.2 °C and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 °C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?” is broken down into a number of easy to follow steps, and 52 words. Since the solution to 107P from 3 chapter was answered, more than 1383 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 107P from chapter: 3 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: Water, Aluminum, heat, beaker, Block. This expansive textbook survival guide covers 19 chapters, and 2045 solutions.

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