Question #f0ab7

1 Answer
Feb 22, 2017

Answer:

#3.96xx10^5J#, rounded to two decimal places.

Explanation:

Taking Specific heat of Aluminum as #904J(kg K)^-1#

Heat required is given by
#DeltaQ=mst#,
where #m,s and t# are the mass, specific heat and rise or gain in temperature of the object; and for change of state as
#DeltaQ=mL#
where #L# is the latent heat for the change of state and
Total heat to be added is #"Heat required to raise the temperature of solid aluminum from "130^@C " to " 600^@C+"Heat required to melt it"#
#=mst+mL#
#=0.45xx904xx(660-130)+0.45xx4.0xx10^5#
#=215604+1.8xx10^5#
#=3.96xx10^5J#, rounded to two decimal places.