How much heat is needed to melt 16.50 kg of silver that is initally at 20 degrees celsius?

Question

this has to do with laten heat.. I tried using Q= mL
do I just do (16.50)(3.33x10^5 J/kg) and ignore the initial temperature? where 16.50 is the mass and 3.33x10^5 is the heat of fusion?
I got 5.0 x 10^6
thanks.

now is the actual value a given from somewhere? or do I have to solve it?

Answer 1

You have 16 kg of silver? And why do you want to melt it down? Have you just stolen it?

Answer 2

Such problems are solved using the equation
Q=mc(t(m)-t(i))+mC (1)
where m is the mass of silver, c its specific heat, C heat of fusion t(m) the melting temperature and t(i) the initial temperature. Under such conditions the final tempertature equates the melting temperature. If you want to overheat the melting to a temperature t(f) you should add
in the right side of (1) term
c(liquid)(t(f)-t(m))
Attention you do not mention the units of some of the involved physical quantities!

Answer 3

just subtract 20 degree celcius from actual value needed to melt ong kg and multiply with 16.50

Answer 4

In thermometr, the quantity of warmth would nicely be calculated utilising the formulation "m*s*t", the place 'm' is the mass of the substance, 's' is the particular warmth of the substance and 't' is the temperature distinction. 'm' of water = a hundred Kg. = a hundred,000 grams 's' of water = a million cal' 't' is comparable to = 20 degree celsius H = one hundred thousand x a million x 20 = 2,000,000 energy =2000 Kilo energy .........=============================...