When 100.0 g block of a metal at 600 oC is plunged into 100.0 g of water (specific heat capacity 4.2 J/g. oC) at 30 oC, the final temperature of both the metal and the water is 80 oC. If no heat is lost to the surroundings, what is the specific heat capacity of the metal in J/g. oC? Give your answer to 2 significant figures.

Explanation:

As we know that,  

        .................(1)

where,

q = heat absorbed or released

= mass of metal = 100.0 g

= mass of water = 100.0 g

= final temperature =

= temperature of metal =

= temperature of water =

= specific heat of metal = ?

= specific heat of water=

Now put all the given values in equation (1), we get

Therefore, the specific heat capacity of metal is

your answer would be a. 12.5 kg

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !