In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Stirring rod A student heats 62.12 grams of platinum to 98.69 °C and then drops it into a cup containıng 78.31 grams of water at 23.37 °C. She measures the final temperature to be 25.15 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of platinum. Metal sample Specific Heat (Pt) = Jg°C.

A fully charged battery contains 0.02 kmol Ag₂O (silver oxide) and 0.02 kmol Zn (zinc). The battery is initially at a temperature of 21°C. The fully charged battery is then discharged for half an hour under adiabatic conditions (no heat leaves the system). During the half hour of being discharged, the electric current from the battery does 200 kJ of work external to the battery system (none of this external work heats the battery). During this half hour, 0.001 kmol of both reactants are consumed in the net cell discharge reaction: Please see the following table for heat capacities and heats of formation. The heats of formation below show the amount of energy (kJ) needed to form one kmole of each component. If the heat of formation is negative, then forming that species releases energy (to do work or provide heat). Therefore, to create one kmole of silver oxide 29000 kJ energy is released and is generated in the battery (for work or heat), and if one kmole of silver oxide decomposes…

6. A 15.0 gram sample of silver metal is heated to 96.7∞C and then dropped into 55.0 grams of water at 23.0∞C.      Assuming that all the heat lost by the silver is absorbed by the water, calculate the final temperature of the silver     and water

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 63.46 grams of aluminum to 97.86 °C and then drops it into a cup containing 76.65 grams of water at 22.09 °C. She measures the final temperature to be 33.20 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of aluminum. Specific Heat (Al) = = J/g °C. Water- Thermometer Metal- sample 2003 Thomson-Brooks/Cole Stirring rod

You work in a chemical plant which recovers gold from gold-plated electrical connectors using heated (Tacid = 55oC) nitric acid.  Once the acid is “used up” it gets piped through the plant to a separate facility for disposal.  During that time, it passes through a cooling chamber to strip the waste heat off the acid for recovery.  The acid passes through the chamber in 6m long, 400mm OD, 360mm ID aluminum tubes. The chamber passes room-temperature air over the tubes at 8 m/s.  Approximately 0.45 cubic meters of acid is processed per hour. a) What is the Reynold’s number of the nitric acid passing through the tube?  Is it turbulent or laminar? b) What is the heat transfer coefficient of the nitric acid to the inside of the aluminum tube? c) What is the heat transfer coefficient of the air over the tube? d) What is the overall heat rate from the nitric acid to the air? e) Based on your answers here, in a gas-liquid heat exchanger, which side of the exchanger are the fins usually on?…

Q3(a) A stream of benzene vapor at 580 °C and 1 atm is cooled and converted to a liquid at 25 °C and latm in a continuous condenser. (i) (ii) Illustrate a completely process path for the above process. Calculate the total enthalpy change for this process.

Magnesium metal, a gray solid, is heated in a crucible in the presence of oxygen. A white powder is collected from the crucible. This is an example of A) a chemical change B) a separation C) a mixture D) a physical change

A CHM student completing the calorimetry experiment mixes 20.0 mL of 1.10 M HCl (aq) with 20.0 mL of 1.05 M NaOH (aq), and observes the temperature increase of 6.611∘∘C.  Assume that the density of each solution is 1.02 g/mL, and the specific heat for the resulting solution is 4.02 J/g∙℃.  Calculate the change in enthalpy for this reaction (ΔHrxn) in kJ/mol H2O.   Use the correct sign (+ or -) and significant figures.

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

METAL Suppose you heat a metal object with a mass of 32.9 g to 96.6 °C and transfer it to a calorimeter containing 100.0 g of water at 17.2 °C. The water and metal reach a final temperature of 22.4 °C. What is the specific heat of the metal in J/g-°C?