How many moles are in 2.5x1022
atoms of CuOH?

1.50 cal

Explanation:

Given data:

Mass of water = 300 g

Initial temperature = 20 °C

Final temperature = 25 °C

Calories needed = ?

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

Solution:

ΔT  = T2 - T1

ΔT  = 25 °C - 20°C

ΔT  =  

Q = m.c. ΔT

Q = 300 g . 4.18j/g. °C . 5°C

Q = 6270 J

J calories:

6270 / 4184 = 1.50 cal