Calculate the amount of heat required or released for each of the following problems. you will
need to refer to your periodic table b-3, and table b-4 in your chemistry reference guide.
3.29) how much heat is required to raise the temperature of 475 grams of solid aluminum from
room temperature (295 k) to liquid aluminum at 1050 k? aluminum melts at 933.47 k.

Q = 322762.5 J

Explanation:

Given data:

Mass of aluminium = 475 g

Initial temperature = 295 K

Final temperature = 1050 K

Heat required = ?

Solution:

Specific heat capacity of Al = 0.900 j/g. K

ΔT  = T2 -T1

ΔT  = 1050 - 295

ΔT = 755 k

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

Q = m.c. ΔT

Q =  475 g × 0.900 j/g. K × 755 K

Q = 322762.5 J

the correct answer to this question is 2