A bar of pure gold is heated to 95.0 degrees Celsius. The specific heat capacity of gold is 1.29 X 10^2. The gold is placed into 500 mL of ethyl alcohol initially at a temperature of 25 Celsius. The final temperature of the mixture is 27.0 Celsius. What is the mass of the gold?

First we have to use conservation of energy, that the heat transferred from gold to the alcohol used to raise the temperature of the alcohol by 2 degrees.                         the heat lost by gold = heat required by the methyl    (m of gold)(C of gold)(dTof gold) = (m of ethyl)(C of ethyl)(dT of ethyl)    where;m of gold is the unknown to be determinedc of gold is the specific heat of gold dT of gold is the change in temperature in goldm of ethyl is the mass of ethyl alcoholC of ethyl is the specific heat of ethyldT is the change in temperature in ethyl alcohol   now                                         mass of gold = unknown                                               c of gold = 129                                  dT of gold = 95 - 25 = 68 degrees                     m of ethyl = density of ethyl * volume of ethyl                              789 X 0.5 X 10^(-3) = 0.3945                                 mass of gold = 0.3945 kg