A student heats 68.15 grams of silver to 98.73 °C and then drops it into a cup containing 78.21 grams of water at 23.04 °C. She measures the final temperature to be 26.47 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.88 J/ °C. Assuming that no heat is lost to the surroundings calculate the specific heat of silver. Specific Heat (Ag) = J/g°C.

When immersed in water, the temperature of a 102.1 gram sample of metal changes from 150.2 0C to 45.2 0C. During this temperature change, the heat of the metal was -10,161 joules. Calculate the specific heat capacity of the metal.

In the laboratory a student finds that it takes 54.9 Joules to increase the temperature of 11.0 grams of solid zinc from 24.0 to 37.6 degrees Celsius. The specific heat of zinc calculated from her data is J/g°C.

We add 3.358 kJ of heat to a calorimeter that contains 50.0 g of water. The temperature of the water and the calorimeter, originally at 22.34 ◦C, increases to 36.74 ◦C. Calculate the heat capacity of the calorimeter in J/◦C. The specific heat of water is 4.184 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.

In the laboratory a student finds that it takes 62.4 calories to increase the temperature of 15.0 grams of solid magnesium from 20.9 to 39.3 degrees Celsius. Based on these data, what is the specific heat of magnesium?

A hot metal weighing 65.0 g was heated to 125 oC and dropped into 75.0 g of water kept at a room temperature of 20.6 oC in a calorimeter. Within a couple of minutes, water’s temperature increased to 26.8 oC and stayed constant at that temperature. If the heat capacity of calorimeter constant is 11.5 J/oC, find the specific heat capacity of the metal.

When 1.75 g of CaCl2 dissolves in 125 g of water in a coffee-cup calorimeter, the temperature increases by 2.44°C. What is the heat change per mole of CaCl2 dissolved in water? Assume that all the heat is absorbed by the water (c = 4.18 J/g·°c).

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 °C to 28.5 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams) of the sample?