The amount of cold water needed to lower the temperature in a container can be calculated using the formula Q = mCΔT, where Q is the heat energy, m is the mass of water, C is the specific heat capacity of water, and ΔT is the desired temperature change. Simply rearrange the formula to solve for m, the mass of water.
The specific heat capacity of water is defined as the amount of heat energy required to raise the temperature of 1 gram of water by 1 degree Celsius. Its value is approximately 4.18 joules/gram °C.
The initial temperature of the water does not affect the amount of cold water needed to lower the temperature in the container. The amount of cold water needed depends on the desired temperature change and the specific heat capacity of water, which remains constant regardless of initial temperature.
Yes, the type of container can affect the amount of cold water needed to lower the temperature. Different materials have varying thermal conductivity, which can affect the rate at which the container transfers heat to the water. This in turn can impact the amount of cold water needed to reach the desired temperature change.
Yes, there is a limit to how much the temperature can be lowered by adding cold water to a container. This is due to the laws of thermodynamics, specifically the law of conservation of energy. The temperature of the water will eventually equalize with the temperature of the surroundings, and adding more cold water will not result in a further decrease in temperature.