Given:
m = 24 g
C = 1 cal/g.oC
Ti = 10 oC
Tf = 20 oC
use:
Q = m*C*(Tf-Ti)
Q = 24.0*1.0*(20.0-10.0)
Q = 240.0 cal
Answer: 240 cal
2. A metal sample having a temperature of 100°C and a mass of 45.2 g was placed in 50 g of water with a temperature of 26°C. At equilibrium, the final temperature was 32.7°C a) How much heat flowed into the water? b) What is the heat capacity of the metal?
A metal sample weighing 43.5 g at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1°C. At equilibrium, the temperature of the water and metal was 33.5°C. What was ΔT for the water? (ΔT = Tfinal - Tinitial) What was ΔT for the metal? Using the specific heat of water (4.184 J/g°C), calculate how much heat flowed into the water. Calculate the specific heat of the metal.
A 150.0-g sample of metal at 80.0°C is added to 150.0 g of H20 at 20.0°C. The temperature rises to 23.3°C. Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal? (Specific heat of H2O is 4.18 J/g. °C.) A) -0.48 J/g. °C B) 0.24 J/g °C C) 0.48 J/g °C D) 0.72 J/g °C E) 0.96 J/g. "C
A metal sample weighinh 45.2 g and at a temperature of 100.0 C was placed in 38.6 g of water in an aluminum calorimeter at 25.2 C. The mass of the calorimeter is 70.4 g and its specific heat is 0.900 J/gC. At equilibrium the temperature of the water, metal and calorimeter was 33.0 C. A. How much heat flowed into the water and calorimeter? Total heat gained = heat gained by calorimeter + heat gained by water OR q=(mass)(s)(changeT)...
A piece of Fe metal with a mass of 0.350 kg at a temperature of 300 °C is added to 1.00 kg of H2O(1) at a temperature of 20 °C. What is the final equilibrium temperature of the H:0(0) and the Fe? The specific heat of the Fe metal is 0.502 J/g.°C and the specific heat of Hh0 is 4.18 Jlg. C.
9. A 48.8 g piece of an unknown metal was heated to 99.8°C, then dropped into a coffee cup calorimeter containing 40.0 g of water at 26.3°C The temperature of the water increased to 30.2°C. How much heat flowed into the water? What is the specific heat of the unknown metal?
12. When 72 g of a metal at 97.0 C is added to 100.0 g of water at 25.0 °C, the final temperature is found to be 29.1 C. What is the specific heat of the metal? (6 pts) 13. Convert the following temperatures. (6 pts) a) 97 0F to oC b) 589 K to oF 14. A hospital patient has an oral temperature of 39.5 °C and weighs 195 Ibs. He is to receive drug, the total dosage of...
A 30.5 g sample of pure metal at 156.7˚C is added to a 0.700 kg of water (specific heat capacity = 4.180 J/˚C g) at 23.0 ˚C. What is the final temperature of the water if the metal is (a) antimony, specific heat capacity of 0.210 J/˚C g (b) iridium, specific heat capacity of 1.30 J/˚C g? Assume all heat is conserved.
1. (10 pts) A 150.0 g sample of a metal at 75.0 °C is added to 150.0 g H20 at 15.0 °C (s.h. = 4.184 J/g °C). The temperature of the water rises to 18.3 °C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water.
1) 150 g of a liquid at 45°C is filled in an insulated metal container at 35°C whose mass is 110 g. The system eventually reaches an equilibrium. Find: (a) the final equilibrium temperature, and (b) estimate total change in entropy of the system (i.e. metal container plus liquid). Specific heat of liquid is 4186 J/kg.Cº and specific heat of metal is 900 J/kg.C. 2) A Carnot engine working between a hot and cool reservoir, extracts 800 J from a...