A piece of unknown metal absorbed 790.24 J of heat as it was heated from 40.0°C to 72.0°C. If the piece of metal weighed 55.0 g, what is the identity of the metal?

Given metal is iron

Explanation:

Given data:

Heat absorbed = 790.24 J

Initial temperature = 40.0 °C

Final temperature = 72.0 °C

Mass of metal = 55.0 g

Identity of metal = ?

Solution:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = 72.0°C - 40.0°C

ΔT =  32 °C

790.24 J = 55 g ×c ×  32 °C

790.24 J = 1760 g. °C  ×c

c = 790.24 J /1760 g. °C

c = 0.449 J/g. °C

The specific heat capacity of iron is 0.449 J/g. °C thus, given metal is iron.

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.