Heat absorbed by the water = Heat loosed by Metal
M(water)*C*(Tf-Ti(water)) = M(metal)*C(metal)*(Ti(metal)-Tf)
150*4.184*(23.8-20) = 35*C(metal)*(100-23.8)
C(metal) = 150*4.184*(23.8-20)/(35*(100-23.8))
Cmetal = 0.89 J/g-C
A piece of metal of mass 35.0 g at 100.0°C was placed in 150.0 g of...
. A 150.0 g sample of a Metal was heated to 95.0°C. When the hot metal was placed into 100.0 g of water in a calorimeter, the temperature of the water increased from 20.0°C to 35.0°C. The specific heat of water is 4.184 J/g °C. a) What is the specific heat of the metal? Kb) What would the final temperature be if the mass of water was 150.0 q?
please help me. Thanks A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
A piece of titanium at 100.0°C was dropped into 50.0 g of water at 20.0°C. The final temperature of the system was 22.6°C. What was the mass of the titanium? Specific heat (J/g°C) titanium 0.54 water 4.184
6. A piece of 155.0 g aluminium metal at 120°C was placed in a constant pressure calorimeter of negligible heat capacity containing 300.0 g of water at 20°C. Calculate the final temperature of the system (the aluminium metal and the water) in °C: given the specific heat of aluminium metal = 0.90 J/g °C, and that of water 4.184 J/g °C
5) A 70.5 gram piece of metal, initially at 255 °C, is rapidly transferred to 100.0 mL of distilled water, which is initially at 19.6 °C. The temperature of the water increases to 30.8 °C. Given that the density of the water = 1.00 g/mL, calculate the specific heat (J/g °C) of the metal. The specific heat of water is 4.184 J/g °C. 9- (SH)(m)(AT) A) 0.632 B) 3.37 C) 5.17 D) 0.0234 E) 0.296
A piece of metal with a mass of 25.5 at 169.9oC is placed in a styrofoam cup containing 35.0 g of water at 24.3oC. Once the system has reached equilibrium, the final temperature of the water is 34.0oC. What is the specific heat of the metal to four significant digits? The specific heat of water is 4.18 J/g-oC.
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.
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 piece of metal with a specific heat of 1.29 J/g°C is heated to 126.6°C and then placed in 133.868 g of water which is at a temperature of 10.9 °C. After a minute, the temperature of the water has stopped changing and is now 45.6°C. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/g°C. Enter...
A 275-g sample of nickel at 100.0°C is placed in 100.0 g of water at 22.0°C. What is the final temperature of the water? Assume no heat transfer with the surroundings. The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C. Hint: The final temp for both the system and surroundings will be the same.