A block of metal weighing 57.58 g is cooled from 100.0°C to 42.16°C with the release of 544.08 joules of heat. From this data,calculate the specific heat of metal.

When immersed in water, the temperature of a 102.1 gram sample of metal changes from 150.2 0C to 45.2 0C. During this temperature change, the heat of the metal was -10,161 joules. Calculate the specific heat capacity of the metal.

In the laboratory a student finds that it takes 54.9 Joules to increase the temperature of 11.0 grams of solid zinc from 24.0 to 37.6 degrees Celsius. The specific heat of zinc calculated from her data is J/g°C.

a 25.31 g sample of a substance is initially at 23.9 °c. after absorbing 2317 j of heat, the temperature of the substance is 103.3 °c. what is the specific heat ( cc ) of the substance?

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 3.50 kg of water at 38.6 °C. During the reaction 131. kJ of heat flows out of the flask and into the bath.Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g^−1K^−1. Round your answer to 3 significant digits.

107 g of Cu at 108.9°C was added to 258.7 g of H2O at 17.4°C.  If the specific heat of copper is 0.389 J/g⋅⋅°C, what is the final temperature of the water and copper?

A solution is made by mixing 260.0 mL of ethanol initially at 15.5 °C with 260.0 mL of water initially at 23.4 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g.°C and the specific heat of water is 4.184 J/g.°C. Tf = °C

How much heat is required to raise the temperature of 25g of water from 25.0°C to 30.0°C? The specific heat of water is 4.184J/g°C.

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 8.60kg of water at 28.2°C. During the reaction 107.kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J·g^−1K^−1.   Round your answer to 3 significant digits.