4. What mass of water would absorb 7.00 × 10² cal of heat if the temperature is increased from 35.0°C to 47.0°C? 5. A 4.00 g sample of a salt is dissolved in 50.0 g of water at 25.00°C. If the specific heat of the resulting solution is 0.970 cal/g °C and if the final temperature of the solution is 34.00°C, calculate the heat of solution of the salt in cal/g.

When you mix two substances, the heat gained by one substance is equal to the heat lost by the other substance. Suppose you place 125 g of aluminum in a calorimeter with 1,000 g of water. The water changes temperature by 2 °C and the aluminum changes temperature by –74.95 °C. A. Water has a known specific heat capacity of 4.184 J/g °C. Use the specific heat equation to find out how much heat energy the water gained (q). B. Assume that the heat energy gained by the water is equal to the heat energy lost by the aluminum. Use the specific heat equation to solve for the specific heat of aluminum. (Hint: Because heat energy is lost, the value of q is negative.) C. Aluminum’s accepted specific heat value is 0.900 J/g °C. Use this value to check your work. Calculate the percent error for the specific heat of aluminum.

A solution is made by mixing 260.0 mL of ethanol initially at 15.5 °C with 260.0 mL of water initially at 23.4 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g.°C and the specific heat of water is 4.184 J/g.°C. Tf = °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 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.

4. A 505 gram piece of copper tubing is heated to 99.0 °C and placed in an insulated vessel containing 59.8 grams of water at 24.8 °C. Assume that the water and the vessel are at the same temperature and that all of the heat released from the copper is absorbed by the water and the vessel. If the vessel has a heat capacity of 10.0 J/K, what is the final temperature of the system when it reaches physical equilibrium?

A 9.13-g sample of vanadium is heated to 99.10 °C and is then placed into 20.0 g water in a calorimeter. The water temperature rises from 20.51 to 24.46 °C. Calculate the specific heat of vanadium.

A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 C. After the salt has completely dissolved, the temperature of the solution is 28.54 C. What is the total heat for the dissolution reaction of the 6.61 g of salt

A 234.66 gram aqueous solution has a specific heat of 4.186 J/gºC. The solution is at 28.1 °C. What is the temperature of the solution in °C after 54.93 kJ of heat has been added to it?