A237.0 g sample of molybdenum metal is heated to 100.10 °c and then dropped into an insulated cup containing 244.0 g of water at 10.00 °c. if the final temperature of the water and metal in the cup is 15.30 °c, then what is the specific heat of molybdenum? (specific heat of water = 4.186 j/g-°c do not add the unit in the answer.

Answer : The specific heat of molybdenum metal is,

Explanation :

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

where,

= specific heat of molybdenum metal = ?

= specific heat of water =

= mass of molybdenum metal = 237.0 g

= mass of water = 244.0 g

= final temperature of water and metal =

= initial temperature of molybdenum metal =

= initial temperature of water =

Now put all the given values in the above formula, we get

Therefore, the specific heat of molybdenum metal is,

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.