How much will the temperature of a cup (183 g) of coffee at 96.1 °C be reduced (in °C) when a 45 g silver spoon (specific heat 0.24 J/g °C) at 24.3°C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same specific heat as water (4.184 J/g °C)

The temperature of an object increases by 39.4 °C when it absorbs 3715 J of heat. Calculate the heat capacity of the object. %3D J/°C The mass of the object is 393 g. Use the table of specific heat values to identify the composition of the object. Substance Specific heat (J/(g °C)) 0.129 silver 0.240 iron 0.444 aluminum 006'0 The object is composed of gold. aluminum.

During an experiment, 25 g of 0.32 M Ca(NO3)2 at 42°C is added to 103 g of 0.82 M HNO3 at 37°C in a calorimeter resulting to the increase in temperature to 78.2°C as Ca(OH)2 is being formed. Considering that the specific heat of the solution and the products are equal to 2.35 J/g°C, calculate the total amount of heat in Joules produced.

A 15.0-mL sample of benzene at 21.0 °C was cooled to its melting point, 5.5 °C, and then frozen. How much energy was given off as heat in this process? (The density of benzene is 0.80 g/mL, its specific heat capacity is 1.74 J/g · K, and its heat of fusion is 127 J/g.)

You add some of the white crystals to a small test tube filled with water. The water in the test tube was initially at room temperature (25˚C). Once the crystals were added and the tube was stirred, the temperature of the solution decreased to about 15˚C and all of the crystals dissolved. what is the change in enthalpy (∆H) for this process?

How many milliliters of water at 31 °C with a density of 1.00 g/mL must be mixed with 95.0 mL (about 6 oz) of coffee at 105 °C so that the resulting combination will have a temperature of 71°C? Assume that coffee and water have the same density and the same specific heat capacity (4.184 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

22.9 mL of an unknown acid was neutralized by mixing it with 50.3 mL of NaOH in an aqueous solution. The final temperature of the solution was 35.2 °C. The initial temperature of the acid and base was 22.0 °C.  Assuming that the density of the solution is 1.00 g/mL and the specific heat is 4.184 J/g°C, what is the heat of neutralization reaction?

A chemist dissolved an 10.8-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 23.9°C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g - °C. %3D =Db Calculate the heat of solution for KOH in kJ/mol. kJ/mol heat of solution =

4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be different if the specific heat of water were that of lead at 0.128 J/gC.