Apiece of copper has a temperature of 75.6 0c. when the metal is placed in 100.0 grams of water at 19.1 0c, the temperature rises by 5.5 0c. what is the mass of the metal?

115.58 g ≅ 115.6 g.

Explanation:

Heat lost by copper (Qc) = Heat gained by the water (Qw) ,

- (Qc) = (Qw).

Qw = m.c.ΔT,

where, Qw is the amount of heat released to water (Q = ??? J).

m is the mass of water (m = 100.0 g).

c is the specific heat capacity of solution (c = 4.18 J/g.°C).  

ΔT is the difference in T (ΔT = final temperature - initial temperature = 24.6°C - 19.1°C = 5.5°C).

∴ Q = m.c.ΔT = (100.0 g)(4.18 J/g.°C)(5.5°C) = 2299 J.

(Qc) = m.c.ΔT,

where, Qc is the amount of heat lost by substance (Qc = - 2299 J).

m is the mass of water (m = ??? g).

c is the specific heat capacity of solution (c = 0.39 J/g.°C).

ΔT is the difference in T (ΔT = final temperature - initial temperature = 24.6°C - 75.6°C = - 51.0°C).

∴ (- 2299 J) = (m)(0.39 J/g.°C)(- 51.0°C).  

∴ m of copper = (- 2299 J)/(0.39 J/g.°C)(- 51.0°C) = 115.58 g ≅ 115.6 g.

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.

i think that the answer is c