Answer:
449.1 g
Explanation:
The second law of thermodynamics states that heat flows from hotter objects to colder ones. Assuming that [tex]Q_1 = 150,000 J[/tex] is the heat given off by a substance in order to melt the ice, we also need to introduce the equation representing the melting of ice:
[tex]Q_2 = \Delta H^o_{fus} m_{ice}[/tex]
Since energy is conserved, the heat given off should be equal to the heat gained:
[tex]Q_1 = Q_2[/tex]
So that the equation becomes:
[tex]\Delta H^o_{fus} m_{ice} = Q_1[/tex]
The enthalpy of fusion of ice is equal to:
[tex]\Delta H^o_{fus} = 334 J/g[/tex]
From here, rearrange the equation for the mass of ice:
[tex]m_{ice} = \frac{Q_1}{\Delta H^o_{fus}} = \frac{150,000 J}{334 J/g} = 449.1 g[/tex]
