A block made of cobalt with a mass of 0.80 kg is heated to 850°C, then dropped into 7.00 kg of water at 11°C. What is the total change in entropy (in J/K) of the block-water system, assuming no energy is lost by heat from this system to the surroundings? The specific heat of cobalt is 420 J/(kg · K), and the specific heat of water is 4,186 J/(kg · K). (Hint: note that dQ = mcdT.) J/K

A block made of cobalt with a mass of 0.80 kg is heated to 850°C, then dropped into 7.00 kg of water at 11°C. What is the total change in entropy (in J/K) of the block-water system, assuming no energy is lost by heat from this system to the surroundings? The specific heat of cobalt is 420 J/(kg · K), and the specific heat of water is 4,186 J/(kg · K). (Hint: note that dQ = mcdT.) J/K