Answer:
Only sketch B has the water molecules in the right form/state that the temperature presented predicts!
Explanation:
N.B - With the initial assumption that all the processes or water states exist at normal conditions of atmospheric pressure and temperature!
In the image attached to this solution, sketch A is at -23°C, sketch B is at 237°C and sketch C is at 60°C.
But for water, it's boiling point is 100°C; meaning that the this is the temperature where water molecules change form from fairly free to move around, almost incompressible liquid state to the gaseous state in which the water molecules (now called steam) are totally free to move around.
Its melting point is 0°C; that is, this is the temperature where the water molecules change form from the orderly solid form (called ice) where motion is totally restricted to only vibrations into the more free liquid state.
This explanation indicates that water molecules at temperatures below 0°C exist in the orderly solid form.
Water molecules at temperatures between 0°C and 100°C exist as the fairly free liquid and at temperatures higher than 100°C, the water molecules exist in the free to move about gaseous state.
In the sketches attached to this solution, sketch A evidently shows the water molecules in the fairly free to move about form (that is, liquid form), but matches this state with a temperature of -23°C which corresponds more to the solid, orderly state of water molecules shown in sketch C. Hence, that is a mismatch.
Sketch B shows water molecules in the very freeing state of gaseous form and rightly matches that form with a temperature way above the boiling point of water, 237°C. Thereby indicating a correct match between temperature and the sketch.
Sketch C however shows water molecules in their very organized solid form but mismatches this form to 60°C which corresponds more to the liquid state sketch in sketch A.
Only sketch B has the water molecules in the right form/state that the temperature presented predicts!
Hope this helps!!!
