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Report (any type)/Brief report
22/09/2021
##0.39″J”/(“g” “”^@”C”)##
A substance’s tells you how much heat much be provided to increase the temperature of ##”1 g”## of that substance by ##1^@”C”##.
The equation that establishes a relationship between how much heat a substance must absorb in order to register a change in its temperature looks like this
##color(blue)(q = m * c * DeltaT)” “##, where
##q## – the amount of heat absorbed
##m## – the mass of the sample
##c## – the of the substance
##DeltaT## – the change in temperature, defined as the difference betwen the final temperature and the nitial temperature
In your case, you know that the temperature of ##”95.4-g”## sample of copper increases from ##25## to ##48^@”C”## after absorbing ##”849 J”## worth of heat.
Rearrange the equation to solve for ##c## and plug in your values
##c = q/(m * DeltaT)##
##c = “849 J”/(“95.4 g” * (48-25)^@”C”) = 0.38693″J”/(“g” “”^@”C”)##
Rounded to two , the number of sig figs you ahve for the two temperatures of the copper sample, the answer will be
##c = color(green)(0.39″J”/(“g” “”^@”C”))##
It’s worth noting that the result matches listed values almost perfectly
http://www.engineeringtoolbox.com/specific-heat-metals-d_152.html
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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