A 3.4 gram piece of metal at a temperature of 95 °C is dropped into a calorimeter filled with 50.0 grams of water at an initial temperature of 23 °C. What is the final temperature of the water and metal when thermal equilibrium is reached? The specific heat of water is 4.184 J/g °C. The specific heat of the metal is 0.49 J/g °C. ​

the answer is 1 i believe

lol for the pointsss

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.