A 20.0 g piece of a metal is heated and place into a calorimeter containing 250.0 g of water initially at 25.0 oC. The final temperature of the water is 31.5 oC. What is the heat change of the metal in joules? The specific heat of water is 4.184 J/goC

Explanation:

By the First Law of Thermodynamics, the piece of metal and water reaches thermal equilibrium when water receives heat from the piece of metal. Then:

Heat change of the metal = -6799 J

Explanation:

Step 1: Data given

Mass of the metal = 20.0 grams

Mass of water = 250.0 grams

Initial temperature of water = 25.0 °C

Final temperature of water = 31.5 °C

Step 2: Calculate the heat change of the metal in joules?

Heat lost =  heat gained

Qlost = -Qgained

Q = m*C*ΔT

m(metal) * C(metal) * ΔT(metal) = -m(water) * C(water) * ΔT(water)

⇒with m(metal) = the mass of metal = 20.0 grams

⇒with C(metal) = the specific heat of meteal = ?

⇒with ΔT(metal) = the change of temperature of the metal = ?

⇒with m(water) = the mass of water = 250.0 grams

⇒with C(water) = the specific heat of water = 4.184 J/g°C

⇒with ΔT(water) = the change of temperature of water = T2 - T1 = 31.5 °C - 25.0 °C = 6.5 °C

The heat change of metal = heat change of water

Q = 250 * 4.184 * 6.5

Q = 6799 J

Heat change of water = 6799 J

Heat change of the metal = -6799 J

step-by-step explanation:

whole numbers, zero or greater

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: