If the same amount of heat is added to 25.0 g of each of the metals, which are all at the same initial temperature, which metal will have the highest final temperature

The metal with the lowest specific heat capacity

Explanation:

Hello, this question can be solved when we compare their specific heat capacities.

Specific heat capacity of a metal /substance is the heat required to raise it's temperature by one degree Celsius.

Mathematically,

Q = mc∇θ

Q = heat energy applied

M = mass of the metal

C = specific heat capacity of the metal

∇θ = (θ₂ - θ₁) which corresponds to the change in temperature of the metal.

In a given experiment of different metals with different specific heat capacities, assuming they're of equal mass and same amount of energy is applied with the same amount of initial temperature, the metal with the lowest specific heat capacity would have the highest final temperature likewise the metal with the highest specific heat capacity would have the lowest final temperature.

The is due to the energy required to raise the temperature of the metal by 1°C

a polar bond is formed when electrons are shared unevenly between atoms

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.