1 mol of water at 10°C is converted into ice at – 10°C. The change in enthalpy for complete conversion is

Question

1 mol of water at \(10^\circ C\) is converted into ice at \(- 10^\circ C\). The change in enthalpy for complete conversion is \(\text{[ Given : }C_p \text{ of water } = x \ JK^{-1} mol^{-1}\) \(C_p \text{ of ice } = y \ JK^{-1} mol^{-1}\) \(\Delta H_{\text{fusion}} = zJ \ ]\)

(1) (–10x – 10y – z)J 

(2) (10x + 10y + z)J 

(3) (x + y – z)J 

(4) 10(x + y – z)J

Answer 1

Correct option is: (1) (–10x – 10y – z)J