Solution Found!
A cook wants to heat 1.35 kg of water from 32.0 °C to 100.0 °C. If he uses the
Chapter 3, Problem 104P(choose chapter or problem)
A cook wants to heat 1.35 kg of water from \(32\ ^{\circ}\mathrm{C}\) to \(100.0\ ^{\circ}\mathrm{C}\). 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.)
Equation Transcription:
Text Transcription:
32 deg C
100.0 deg C
Questions & Answers
QUESTION:
A cook wants to heat 1.35 kg of water from \(32\ ^{\circ}\mathrm{C}\) to \(100.0\ ^{\circ}\mathrm{C}\). 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.)
Equation Transcription:
Text Transcription:
32 deg C
100.0 deg C
ANSWER: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.
q = heat
m = Mass of the substance
C = Specific heat capacity of a substance.