Question: The specific heat of copper metal is 0.385 J/(g° C). How many J of heat are necessary to raise the temperature of a 1.42 kg block of copper from 25.0°Сto 88.5°C? a) 547 J b) 1.37 x 104) c) 3.47 x 104 J d) 34.7 J e) 4.74 x 104 J X

3.47x 10^4

Explanation:

the energy required to raise the temperature is = the mass in grams x the specific heat capacity of copper metal x (final temperature - initial temperature)

1.42 x 10^3 x 0.385 x (88.5-25)= 3.47 x 10^4

dynamic equilibrium is the answer.

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.