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A cook wants to heat 1.35 kg of water from 32.0 °C to 100.0 °C. If he uses the

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

Solution for problem 104P 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 104P

Problem 104P

A cook wants to heat 1.35 kg of water from 32.0 °C to 100.0 °C. If he uses the combustion of natural gas (which is exothermic) to heat the water, how much natural gas will he need to burn? Natural gas produces 49.3 kJ of heat per gram. (For the sake of simplicity, assume that the transfer of heat is 100% efficient.)

Step-by-Step Solution:

Problem 104P

A cook wants to heat 1.35 kg of water from 32.0 °C to 100.0 °C. If he uses the combustion of natural gas (which is exothermic) to heat the water, how much natural gas will he need to burn? Natural gas produces 49.3 kJ of heat per gram. (For the sake of simplicity, assume that the transfer of heat is 100% efficient.)

                                                Step by step solution

Step 1 of 2

The relation between the amount of heat added to a given amount of the substance and the corresponding temperature is as follows.

                                                   ..................................(1)

q = heat

m = Mass of the substance

C = Specific heat capacity of a substance.

Step 2 of 2

Chapter 3, Problem 104P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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A cook wants to heat 1.35 kg of water from 32.0 °C to 100.0 °C. If he uses the