Please answer step-by-step with solutions:
A 150.0 iron bar at 330 degrees C is put in 1.00 kg water at 20.0 degrees C. What is the final temperature of the bar?
(Hint: bar and water will be the same at the end.)
Cs = 0.45J/(grams degree C) for iron
Cs = 4.18J/(grams degree C) for water
Assuming all of the heat released from the iron bar absorbed by water, you can than set up the following two equations:
For the heat released by the iron ...
The solution is given step-by-step to solve for T2.
Calorimetry and Hess' Law
Detailed work would be very helpful; the math involved in this gets me confused, but I'm not sure where I have been going wrong. If work is handwritten, please do not write in cursive for I have problems reading it.
1. The mass of a substance is 200gm and its specific heat is 0.09. How much heat is required to raise the temperature of the substance from 20°C to 90°C?
2. The heat capacities of mercury and glass are the same. The density of mercury is 13.6gm/cc and the density of glass is 2.5gm/cc. If the specific heat of mercury is 0.03, what will be the specific heat of glass?
3. A body of mass 100gm is heated to 122° C and then quickly dropped into a copper calorimeter of mass 50gm. The calorimeter contains 300gm of water at 28° C. The final temperature of the system becomes 30° C. What is the specific heat of the body if the specific of copper is 0.09?
4. Use the following information to determine the enthalpy (?H°) of the reaction for:
NO2 (g) + (7/2) H2 (g) --> 2H2O (l) + NH3 (g)
Using the following two equations:
2NH3 (g) --> N2 (g) + 3H2 (g) ?H° = +92 kJ
(1/2) N2 (g) + 2H2O (l) --> NO2 (g) + 2H2 (g) ?H° = +170kJ
5. The compound carbon suboxide, C3O2, is a gas at room temperature. Use the data supplied the calculate the heat of formation of carbon suboxide.
2CO (g) + C (s) --> C3O2 (g) ?H° = +127.3 kJ
CO(g) ?H° = -110.5 kJ