The temperature of a piece of copper with a mass of 95.4 g increases from 25C to 48C when the metal absorbs 849 J of heat. What is the specific heat of copper?

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    ##0.39J/(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) = 0.38693J/(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)(0.39J/(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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