. A piece of an iron metal of unknown mass is heated to 325.9 o C and then placed in a styrofoam coffee cup containing 225.2 mL of water at 22.15 o C. After the system comes to thermal equilibrium, the temperature of the water is 29.65 o C. Assuming that no heat is lost to the cup or the surroundings, determine the mass of the iron metal. The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C. The density of water is 1.000 g/mL.

As a system increases in volume, it absorbs 55.0 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.540 atm. The final volume of the system is 58.2 L. What was the initial volume of the system if the internal energy of the system decreased by 103.4 J?

A particular container holds 3.77 mol of neon gas. The volume of this container can be altered by sliding a piston in or out. The volume is changed from 8.60 L to 12.20 L while at the same time the temperature is changed from 303 K to 345 K. The molar heat capacity, Cym, for neon is 12.47 J/(mol · K). Assume that this value will not change over the given temperature range. What is the change in entropy for the gas? AS = J/K TOOLS x10 MacBook Pro

A 5.1-gram piece of gold jewelry isremoved from water at 100.0°C and placed in a coffee-cup calorimeter containing 16.9 gof water at 22.5°C (specific heat of water is 4.184 J/g · °C). The equilibrium (final)temperature of the water and jewelry is 23.2°C. The calorimeter constant is known fromcalibration experiments to be 1.54 J/°C. What is the specific heat (in J/g · °C) of this pieceof jewelry? If the tabulated value of the specific heat of gold is 0.129oC, is the jewelrypure gold?

A 32.1 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 25.8°C. Calculate the mass of water in the calorimeter.

A sample of a gas was compressed from a volume of 1.00 L to 0.250 L against a constant pressure of 1.10 atm. What is the change in internal energy if the system gives off 132 J of heat to the surroundings? 1 L atm = 101.3 J

A student has calibrated his/her calorimeter and finds the heat capacity to be 14.8 J/°C. S/he then determines the molar heat capacity of aluminum. The data are: 25.7 g Al at 100.0°C are put into the calorimeter, which contains 99.8 g H20 at 18.5°C. The final temperature comes to 22.6°C. Calculate the heat capacity of Al in J/mol-°C

A 44.0 g sample of unknown metal at 99.0°C was placed in a constant-pressure calorimeter containing 80.0 g of water at 24.0°C, the final temperature of the system was found to be 28.4°C. Calculate the specific heat of the metal.

A 37.7 g. piece of an unknown metal is heated up 43.5 °C when given 1,095.4 J of heat.  What is the specific heat capacity of the metal?

A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C