A 25.0 g sample of silver metal was heated to 170 degrees C and then placed in a calorimeter holding 50.0 g of water at 20.0 degrees C. The temperature of the water in the calorimeter rose to 24.1 degrees C. Calculate the specific heat of silver.

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.79 kg sample of a pure substance from 9.1 °C to 17.6 °C. The experiment shows that 1.6 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits.

A chunk of lead at 91.7°C was added to 400.0 g of water at 15.5°C. The specific heat of lead is 0.129 J/g°C, and the specific heat of water is 4.18 J/g°C. When the temperature stabilized, the temperature of the mixture was 19.4°C. Assuming no heat was lost to the surroundings, what was the mass of lead added?

A hot 101.5 g lump of an unknown substance initially at 157.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 36.1 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. O zinc O graphite O tungsten O titanium O rhodium O aluminum Substance Specific heat (J/(g-°C)) 0.897 0.709 0.243 0.523 0.132 0.388 4.184 aluminum graphite rhodium titanium tungsten zinc water