Exam 11: Liquids, solids, and Intermolecular Forces

Define viscosity.

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 80.0 °C is ________ kJ.The specific heats of ice,water,and steam are $2.09 \mathrm { Jg } ^ { - 1 } { } ^ { \circ } \mathrm { C } ^ { - 1 }$ $4.18 \mathrm { Jg } ^ { - 1 } { } ^ { \circ } \mathrm { C } ^ { - 1 }$ and $1.84 \mathrm { Jg } ^ { - 1 } { } ^ { \circ } \mathrm { C } ^ { - 1 }$ respectively.For $\mathrm { H } _ { 2 }$ O, $\Delta _ { \text {fus } } H$ = 6.01 kJ mol^-1,and $\Delta _ { \text {vap } } H = 40.67 \mathrm {~kJ} \mathrm {~mol} ^ { - 1 }$ .

From the phase diagram of benzene given below,predict the temperature at triple point.

Which of the following forms a molecular solid?

Define the boiling point of a liquid.

Give the change in condition to go from a liquid to a gas.

Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.