use the fomula for Heat transfer Q = mcDT
using the principle of calorimetry
45* 4.186* (T-36) = 100 *4.186 * (100-T)
T = 80.13 deg C
Calculate the final temperature of the water from the following heat transfer experiment. 45 g of...
What will be the final temperature of the water in an insulated container as the result of passing 6.00 g of steam [H2O(g)] at 100.0∘C into 100.0 g of water at 23.0 ∘C? (ΔvapH∘=40.6kJ/molH2O) Express your answer in degrees Celsius to three significant figures.
1. Calculate the final temperature that results when a 12.8 g sample of water at 23.1 ∘C absorbs 885 J of heat. Express your answer in degrees Celsius to three significant figures. 2.Calculate the final temperature that results when a 1.63 kg sample of platinum at 78.4 ∘C gives off 1.15 kcal of heat (specific heat of Pt=0.032cal g^−1∘C^−1) Express your answer in degrees Celsius to two significant figures.
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.
A lead block with a mass of 46.5 g at a temperature of 76.98 degrees celsius was placed into a calorimeter containing 100.0 mL of water at a temperature of 20.6 degrees celsius. What is the equilibrium temperature if the specific heat of water is 4.184 J/g and the specific heat of lead is 0.158 J/gdegreeC?
If the temperature of 100.0 mL of water rises from 25.0°C to 32.0°C, how much heat was added? Assume the density of water is 1.00 g/mL and the specific heat capacity of the water is 4.184 J/g°C. Include units and use the correct number of significant figures. Define the terms "exothermic" and "endothermic". What is the sign of AH associated with these two terms? Exothermic: Endothermic
Which of the following processes will result in the lowest final temperature of the metal–water mixture at when thermal equilibrium is reached? The specific heat capacity of cobalt is 0.421 J/(g·°C). The specific heat capacity of water is 4.184 J/(g·°C). a. the addition of 100 g of cobalt at 95°C to 80 mL of water at 25°C in an insulated container b. the addition of 100 g of cobalt at 95°C to 100 mL of water at 25°C in an...
521.8 J of heat was added to 8.00 g of water. The final temperature of the water was measured to be 64.2oC. What was the initial temperature of the water? (specific heat capacity of water = 4.184 J/goC)
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K.
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K
4. Heat transfer: q = mass x Cs x ΔT and –qreaction = +qsolution a. A piece of metal with a mass of 8.6 g was heated to 100.0°C and dropped into a coffee cup calorimeter containing 402.4 g of water at 25.0°C. If the temperature of the water and the metal at thermal equilibrium is 26.4°C, what is the specific heat of this metal in J/g°C? b. How much heat energy must be added in order to boil a...