Why is an ice cube at 0°C more effective in cooling soft drink than the same mass of water at0°C?
Because ice can absorb more heat from the soft drink to change its state from ice to water (latent heat), than water only.
If you use the equation for heat released/absorbed,
Let T2 = final temperature of ice (assume it's above 0°C, so it became water at some temp > 0°C)
Let T1 = initial temperature of ice (which is 0°C
Q(absorbed by ice) = latent heat + sensible heat
Q(absorbed by ice) = m*Lf + m*c*(T2 - 0)
while if water only,
Q(absorbed by water) = m*c*(T2 - 0)
Q absorbed by ice is also the Q released by soft drink.
Hope this helps :)
Because ice absorbs more heat than water
An ice cube at 0°C is more effective in cooling a soft drink than an equal mass of water at the same temperature because of the process of phase change. When the ice cube is added to the soft drink, it continues to absorb heat from the surrounding environment in order to melt and raise its temperature to 0°C. This process, called latent heat of fusion, requires a significant amount of energy.
On the other hand, when water at 0°C is added to the soft drink, it does not undergo a phase change. It simply mixes with the soft drink and reaches an equilibrium temperature. Since the water does not absorb additional energy to melt, it has a lower cooling effect compared to the ice cube.
In summary, the ice cube's ability to absorb heat during the phase change from solid to liquid makes it more effective in cooling the soft drink compared to an equal mass of water at the same temperature.
An ice cube at 0°C is more effective in cooling a soft drink than the same mass of water at 0°C because the ice cube undergoes a phase change while melting, which requires the absorption of a significant amount of heat energy. This process is called latent heat of fusion.
When you add an ice cube to a soft drink, the ice cube absorbs heat from the surrounding environment, including the soft drink itself. In order for the ice cube to melt, it must absorb enough heat energy to overcome the bonding forces between its molecules and transition from a solid to a liquid state.
On the other hand, the water at 0°C does not undergo a phase change, as it is already in the liquid state. It can still absorb some heat from the soft drink, but it cannot absorb as much energy as the ice cube because it does not require a phase change.
Therefore, the ice cube, despite being at the same temperature as the water, is more effective in cooling the soft drink because it absorbs more heat energy during the phase change from solid to liquid. This significantly lowers the temperature of the soft drink, making it colder more quickly.