calorimetry
A 50.0 g sample of water at 25.0 °C is heated with a 100.0 g piece of metal at 150.0 °C. Assuming no heat is lost to the surroundings and that the specific heat capacity of water is 4.18 J/g°C and the specific heat capacity of the metal is 0.385 J/g°C, determine the final equilibrium temperature of the system.
44.4 degrees Celsius
A 2.00 g sample of a hydrocarbon is combusted in a bomb calorimeter. The temperature of the calorimeter increases from 25.00 °C to 30.00 °C. If the calorimeter has a heat capacity of 5.00 kJ/°C, calculate the heat of combustion of the hydrocarbon in kJ/g
-12.5 kJ/g
A system absorbs 300 J of heat and does 100 J of work on the surroundings. Calculate the change in internal energy of the system
200 J
Name N2O3
Dinitrogen trioxide
A 75 g piece of an unknown metal is heated to 150 °C and then placed in a calorimeter containing 200 g of water at 20 °C. The final temperature of the water is 25 °C. Calculate the specific heat capacity of the metal. (Assume no heat is lost to the surroundings.)
0.446 J/g(degrees celcius)
A 3.00 g sample of silicon dioxide is burned in a bomb calorimeter, resulting in a temperature increase of 4.50 °C. The calorimeter has a heat capacity of 10.0 kJ/°C. Calculate the heat of combustion of the compound in kJ/mol.
901.21 kJ/mol
A 200 g block of aluminum (specific heat = 0.897 J/g°C) is heated from 20 °C to 100 °C. Calculate the heat absorbed by the aluminum block.
14352 J
Name Cl2
Chlorine gas
151.6 g of an unidentified solid at 372.2 K is dropped in a container with 420.9 g of water at 321.3 K. The system comes to thermal equilibrium at 328.2 K. The specific heat capacity of water is 4.184 J/(g·K). What is the specific heat capacity of the unknown solid?
1.82 J/(g)(K)
A 5.00 g sample of a new fuel is burned in a bomb calorimeter, causing the temperature of the calorimeter to rise from 25.00 °C to 32.50 °C. The calorimeter has a heat capacity of 12.0 kJ/°C. Calculate the heat of combustion of the fuel in kJ/g.
- 18 kJ/g
A gas in a piston expands from a volume of 2.0 L to 5.0 L against a constant external pressure of 1.0 atm. Calculate the work done by the gas during the expansion. (Use the conversion 1 L·atm = 101.3 J.)
-304 J
the formula for cobalt (lll) chloride
CoCl3