A 59.7 g piece of metal that had been submerged in boiling water was quickly transferred into 60.0 mL of water initially at 22.0 °C. The final temperature is 28.5 °C. Use these data to determine the specific heat of the metal. Use this result to identify the metal.

A metal object with mass of 20.5 g is heated to 97.0 °C and then transferred to an insulated container containing 86.8 g of water at 20.5 °C. The water temperature rises and the temperature of the metal object falls until they both reach the same final temperature of 23.6 °C. What is the specific heat of this metal object? Assume that all the heat lost by the metal object is absorbed by the water.

A 93.82 g bar of iron was heated to 98.4 °C and then dropped into 38.1 mL of water at 15.3 °C.  The temperature of the water increased to a maximum of 32.7 °C.  Calculate the specific heat capacity of iron.  Assume that the density of water is 1.00 g/mL. heat capacity (J/g°C)

The specific heat of a substance is the amount of heat required to raise the temperature of one gram of the substance by one degree Celsius. The relationship between the amount of heat gained or released by a substance and the change in temperature of the substance is given by the equation ?=??Δ?q=m⁢s⁢Δ⁢T where ?q is the heat gained or released, ?m is the mass of the substance, ?s is the specific heat of the substance, and Δ?Δ⁢T is the change in temperature. 1. Rearrange the equation to solve for ?. 2. When a substance with a specific heat of 0.635 J/g⋅∘C0.635 J/g⋅∘C is heated from 25.2 ∘C25.2⁢ ∘C to 71.4 ∘C,71.4⁢ ∘C, it absorbs 422 J422 J of heat. Calculate the mass of the substance.