Answer:
Q = -15363.65 J
Explanation:
Given data:
Number of moles of water = 2.0 mol
Initial temperature = 101°C
Final temperature = -1.0°C
Total energy lost = ?
Solution:
Mass of water:
Mass = number of moles × molar mass
Mass = 2 mol × 18 g/mol
Mass = 36 g
Heat lost:
specific heat capacity of water is 4.184 J/g.°C
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
ΔT = -1.0°C - 101°C
ΔT = -102°C
Q = 36 g × 4.184 J/g.°C × -102°C
Q = -15363.65 J
Negative sign show heat is released.
