Question

Total enthalpy change for freezing of 1 mol water at 10°C to ice at -10°C is ______ (Given: $ \Delta_{\text{fus}}H = x \, \text{kJ/mol} $, $ C_p[\text{H}_2\text{O}(l)] = y \, \text{J mol}^{-1} \text{K}^{-1} $, and $ C_p[\text{H}_2\text{O}(s)] = z \, \text{J mol}^{-1} \text{K}^{-1} $)

• A. \( -x - 10y - 10z \)
• B. \( -10(100x + y + z) \)
• C. \( 10(100x + y + z) \)
• D. \( x - 10y - 10z \)

Hint:

Always ensure that the units are consistent when combining enthalpy changes due to different processes. Convert values as necessary.

Answer 1

The Correct Option is B

To find the total enthalpy change, we need to consider both the freezing process and the cooling of the substance: 
1. Freezing process: The enthalpy change for freezing is \( \Delta_{\text{fus}}H = -x \), since freezing is an exothermic process. 
2. Cooling of liquid water: The enthalpy change for cooling the water from 10°C to 0°C is calculated using the specific heat capacity of liquid water: \[ \Delta H_1 = -10y \] 
3. Cooling of ice: The enthalpy change for cooling the ice from 0°C to -10°C is calculated using the specific heat capacity of ice: \[ \Delta H_2 = -10z \] 
Thus, the total enthalpy change can be expressed as: \[ \Delta H = -x - 10y - 10z \] The term \( x \) is given in kJ/mol and should be multiplied by 100 to convert it to J/mol to match the units of \( y \) and \( z \) (which are in J/mol·K). 
Thus the correct expression for the total enthalpy change is: \[ \Delta H = -10(100x + y + z) \]