Astudent carried heated a 25.00 g piece of aluminum to a temperature of 100°c, and placed it in 100.00 g of water, initially at a temperature of 10.0°c. determine the final temperature of the system (aluminum and water). useful data: the specific heat of water is 4.18 j/(g°c) the specific heat of aluminum is 0.900 j/(g°c)

The final temperature of the system is 14.6 °C

Explanation:

Step 1: Data given

mass of the aluminium = 25.00 grams

mass of the water = 100.00 grams

Initial temperature of aluminium = 100 °C

Initial temperature of water = 10.0 °C

Specific heat of water = 4.18 J/g°C

Specific heat of aluminium 0.900 J/g°C

Step 2: Heat transfer

Loss of Heat of the Metal = Gain of Heat by the Water

Qmetal = -Qwater

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

25*0.900*(T2-100) = - 100*4.18 * ( T2 - 10)

2250 - 22.5T2 = 418T2 - 4180

T2 =14.6 °C

The final temperature of the system is 14.6 °C

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.