Question

The specific heat of silver is 0.0565 cal/g°C. Assuming no loss of heat to the surroundings or container, calculate the final temperature when 100.0 g of silver at 40.0 °C is immersed in 60.0 g of water (cs = 1.0 cal/g°C ) at 10.0 °C.

Answer 1

To calculate the final temperature when silver is immersed in water, we can use the principle of heat transfer. The heat lost by the silver is equal to the heat gained by the water. We can use the equation q = mcΔT, where q is the heat transferred, m is the mass, c is the specific heat, and ΔT is the change in temperature.

To calculate the final temperature when silver is immersed in water, we can use the principle of heat transfer. The heat lost by the silver is equal to the heat gained by the water. We can use the equation q = mcΔT, where q is the heat transferred, m is the mass, c is the specific heat, and ΔT is the change in temperature.

For the silver, we have qsilver = msilvercsilverΔTsilver. For the water, we have qwater = mwatercwaterΔTwater. Since there is no loss of heat to the surroundings or container, qsilver = -qwater.

Given the mass and initial temperature of the silver and water, we can calculate the final temperature using the equation:

ΔTsilver = -(mwatercwater(Tfinal-Tinitial)/(msilvercsilver)