How much heat, in joules and in calories, must be added to a 75.0- g iron block with a specific heat of 0.449 j/g degree cecius to increas its temperature from 25 degree celcius to its melting temperature of 1535 dgree celcius?

The heat required by iron is 50849.25 Joules or 12152.97 Cal.

Explanation:

To calculate the amount of heat released or absorbed, we use the equation:

where,

q = heat absorbed

m = mass of iron = 75 g

c = specific heat capacity of iron = 0.449 J/g.°C

= change in temperature =

Putting values in above equation, we get:

Converting the value from joules to calories, we use the conversion factor:

1 J = 0.239 Cal

So,

Hence, the heat required by iron is 50849.25 Joules or 12152.97 Cal.

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."

c (diamond),

sio2 (quartz)