Question

A sample of nickel is heated to 99.8C and placed in a coffeecup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.

Answer 1

Answer:

The mass of the nickel sample is 28.35 °C

Explanation:

Step 1: Data given

Mass of water = 150 grams

Initial temperature of nickel = 99.9 °C

Initial temperature of water 23.5 °C

Final temperature of water and nickel = 25 °C

Specific heat capacity of nickel = 0.444 J/g°C

Specific heat capacity of water = 4.184 J/g°C

Step 2: Calculate mass of nickel

heat lost by nickel= heat gained by the water

Q = m*c*ΔT

Qnickel = -Qwater

m(nickel)*c(nickel)*ΔT(nickel) = -m(water) * c(water) *ΔT(water)

m(nickel) * 0.444 J/g°C *(25°C - 99.8°C) = -150 grams* 4.184 J/g°C * (25-23.5)

m(nickel) * (-33.2112) = -941.4

m(nickel) = -941.4 / -33.2112

m(nickel) = 28.35 °C

The mass of the nickel sample is 28.35 °C