Asample 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.

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

answer; protein;

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.