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fibrown
Group Title
Which of the following describes an exothermic reaction?
Thermal energy is absorbed by the system.
Thermal energy is absorbed by the surroundings.
Thermal energy is not transferred.
The initial and final temperatures of the system remains the same
What is the specific heat of a substance if 12.6 grams of the substance requires 0.119 kilojoules of heat to increase the temperature by 5.9 degrees Celsius?
1.6 x 100 J/g·°C
1.6 x 10−3 J/g·°C
1.6 x 103 J/g·°C
6.2 x 10−1 J/g·°C
Can someone help please !!!
 one year ago
 one year ago
fibrown Group Title
Which of the following describes an exothermic reaction? Thermal energy is absorbed by the system. Thermal energy is absorbed by the surroundings. Thermal energy is not transferred. The initial and final temperatures of the system remains the same What is the specific heat of a substance if 12.6 grams of the substance requires 0.119 kilojoules of heat to increase the temperature by 5.9 degrees Celsius? 1.6 x 100 J/g·°C 1.6 x 10−3 J/g·°C 1.6 x 103 J/g·°C 6.2 x 10−1 J/g·°C Can someone help please !!!
 one year ago
 one year ago

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chmvijay Group TitleBest ResponseYou've already chosen the best response.0
what is exothermic reaction :)
 one year ago

fibrown Group TitleBest ResponseYou've already chosen the best response.0
Im not sure its last minute chemistry work for school . Im getting confused and cant find the answer
 one year ago

emcrazy14 Group TitleBest ResponseYou've already chosen the best response.3
An exothermic reaction is one where thermal energy is given out or you could say lost by the system. So option 2 is correct i.e thermal energy is absorbed by surroundings.
 one year ago

emcrazy14 Group TitleBest ResponseYou've already chosen the best response.3
For the second question, do you know this formula? \[E=mc \Delta \theta \] where E= thermal energy required m= mass c= specific heat capacity \[\Delta \theta \]= change in temperature Rearranging the equation, you get \[c= E/ m \Delta \theta \] Now you can plug in the values to get your answer.
 one year ago

mathslover Group TitleBest ResponseYou've already chosen the best response.0
Good work emcrazy14. And @fibrown : \(\LARGE{\textbf{Welcome to OpenStudy!}}\)
 one year ago

emcrazy14 Group TitleBest ResponseYou've already chosen the best response.3
Thank you! :)
 one year ago
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