1. How much heat must be added to a 38-g sample of aluminum to increase its temperature by 250.0°C? The specific heat capacity for aluminum is 0.902 J/g °C.

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.

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