if 48.0 grams of water at 78.0 degrees C is added to 75.0 grams of water at 42.0 degrees Celsius what is the final temperature?
if 48.0 grams of water at 78.0 degrees C is added to 75.0 grams of water...
20 grams of ice at -12 degrees celsius is added to 300 grams of water at 30 degrees celsius. When equilibrium is reached, what is the temperature in celsius of the water?
When 55.0 grams of metal at 75.0°C is added to 100. grams of water at 14.0°C, the temperature of the water rises to 17.5°C. Assume that no heat is lost to the surroundings. What is the specific heat of the metal? The specific heat of water is 4.184 J/g·°C.
155 grams of ice at -10.0 degrees celsius is added to 1.17 kg of water at 70.0 degrees celsius and mixed together in thermal isolation until they come to equilibrium. The specific heat of ice is 2010 J/kgC. The specific heat of water is 4186 J/kgC. The latent heat of fusion for water is 3.34x10^5 J/kg. The latent of vaporization for water is 2.26x10^6 J/kg. What is the final equilibrium. The answer is 51.9 celsius. I just need the steps...
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C. a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C. b) What is the total heat needed to melt the 75g of ice? c) What is the total amount of heat required to raise the...
50 grams of water whose temperature is 46°Celsius are added to a thin glass containing 720 grams of water at 20°Celsius (about room temperature). What is the final temperature of the water?
A .500g sample of KCL is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved per mol of KCL?
A .500g sample of KCl is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved in the dissolution of .500g KCl, assuming the heat capacity of the solution is 4.184J/g degrees celsius?
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 12.16 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C). (HINTS: Recall that the q of a system is equal to the -q of the surroundings. So you can set up two equations here: one for the loss...
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 14.37 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius Calculate the specific heat of the metal (The specific heat of water is 4.184J'g'C). (HINTS Recall that the qof a system is equal to the of the surroundings So you can set up two equations here one for the loss of heat from...
5000 Joules of heat are added to 100 grams of water at 30 Celsius. Calculate the final temperature. Cpwater = 4.184 J/g C