27-gram piece of metal at 144  oC is dropped into 86 grams of water at 29 oC.  The water temperature rose to 37 oC.  Calculate the heat change of the metal in Joules.  (DO NOT PUT UNITS IN YOUR ANSWER.)  Assume that all of the heat lost by the metal is transferred to the water and no heat is lost to the surroundings.  The specific heat of water is 4.184 J / g oC

How much heat (in kilojoules) is gained by 294 grams of water that is warmed from 25.00C to 57.00C? The specific heat of water is 4.184 J/(g 0C).

A 33.6-g piece of silver initially at 46.5 °C is submerged into 162.4 g of water at 12.3 °C. What is the final temperature of the metal once the metal and water reaches thermal equilibrium? The specific heats of silver and water are 0.235 J/g·°C and 4.18 J/g·°C, respectively. 29.4 °C 10.4 °C 11.0 °C 12.7 °C 21.0 °C

How much heat (in Joules) is gained by 157 grams of water thát is warmed from 25.0 °C to 74.0°C? The specific heat of water is 4.184 J g °C

How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.

A sheet of metal weighing 275-g is heated to 100.0 °C and placed flat in 100.00 g bucket of water at 22.0 °C. What is the final temperature of the combined substances? Assume that no heat is lost to the surroundings. The specific heat capacity of the metal is 0.444 J/g.°C . The specific heat of water is 4.184 J/g.°C. Select one: O a. 61.0 °C Оъ. 82.4 °С O c. 79.2 °C d. 40.8 °C × О е. 39.6 °C

The temperature of 34.7 g H2O changes from 27 °C to 53 °C. What is the heat associated with this change? Is heat flowing into or out of the water? How do you know?

Suppose a boil water notice is sent out advising all residents in the area to boil their water before drinking it or using it for cooking. You need to boil 18.0 L of water using your natural gas (primarily methane) stove. What volume of natural gas is needed to boil the water if only 10.1% of the heat generated goes towards heating the water. Assume the density of methane is 0.668 g/L, the density of water is 1.00 g/mL, and that the water has an initial temperature of 21.4 °C. Enthalpy of formation values can be found in this table. Assume that gaseous water is formed in the combustion of methane.

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 15.2 g, and its initial temperature is −13.9 ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.9⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.   Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H 2 O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) *  Specific heat of liquid H 2 O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) *  Specific heat of gaseous H 2 O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) *

What will be the final temperature when a 25.0 g block of aluminum (initially at 25 °C) absorbs 10.0 kJ of heat? The specific heat of Al is 0.900 J/g· degrees C.