ThermodynamicsHard
Question
The heat capacity of liquid water is 75.6 J/K-mol, while the enthalpy of fusion of ice is 6.0 kJ/mol. What is the smallest number of ice cubes at 0°C each containing 9.0 g of water needed to cool 500 g of liquid water from 20°C to 0°C?
Options
A.1
B.7
C.14
D.21
Solution
Heat lost by water = Heat gained by ice
$\text{Or, 500} \times \frac{75.6}{18} \times 20 = (N \times 9) \times \frac{6000}{18} \Rightarrow N = 14$
Create a free account to view solution
View Solution FreeMore Thermodynamics Questions
If one mole of a monoatomic gas ($\gamma$ = 5/3) is mixed with one mole of a diatomic gas ($\gamma$ = 7/5), then the val...The ΔG in the process of melting of ice at −15°C and 1 atm, is...Two moles of an ideal monoatomic gas is heated from 27°C to 627°C, reversibly and isochorically. The entropy of gas...The law of equipartition of energy is applicable to the system whose constituents are...Entropy change for an adiabatic reversible process is ?...