An 87.0-g piece of iron whose temperature is 73.8 °C (347.0 K) is placed in a beaker containing 300 g of water at 18.6 °C (291.8 K). When thermal equilibrium is reached, what is the final temperature? (Assume no energy is lost to warm the beaker and its surroundings.) The specific heat of iron is 0.449 J/g∙K, and the specific heat of water is 4.184 J/g∙K. K

During an experiment, 25 g of 0.32 M Ca(NO3)2 at 42°C is added to 103 g of 0.82 M HNO3 at 37°C in a calorimeter resulting to the increase in temperature to 78.2°C as Ca(OH)2 is being formed. Considering that the specific heat of the solution and the products are equal to 2.35 J/g°C, calculate the total amount of heat in Joules produced.

Calculate the heat (q) for 195 grams of pure water heated from a temperature of 25.0 °C to 77.5 °C.The specific heat of water is 4.184 J/(g°C).

In a coffee-cup calorimeter, 110.0 mL of 1.3 M and 110.0 mL of 1.3 M are mixed. Both solutions were originally at 22.2°C. After the reaction, the final temperature is 30.9°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

A sample of silver metal is heated to 100.1 °C in a hot water bath until thermal equilibrium is reached. The sample is quickly transferred to 52.483 g of water at 20.3 °C contained in a calorimeter. When thermal equilibrium is reached at 25.1 °C, what isthe mass of this silver metal? (specific heat of water: 4.184 J / gram●°C)

150. g of water (Cs = 4.184 J/g°C) at 20.0 °C is added to a coffee cup calorimeter. A 35.0 g sample of silver (Cs = 0.129 J/g°C) is then placed into the water.  At thermal equilibrium, the temperature of the calorimeter is 22.07 °C.  What was the initial temperature of the silver sample?

IV (intravenous) solutions are mixtures of sugars, salts and other aqueous solutes fed directly to a patient's veins. If an IV solution is 5.0% glucose by mass, how many grams of solid glucose would be require to prepare 60.0 milliliters (ml) of the solution? Assume the density of the solution is 1.0 g/ml

In a coffee-cup calorimeter, 120.0 mL of 1.0 M NaOH and 120.0 mL of 1.0 M  HCl are mixed. Both solutions were originally at 26.1°C. After the reaction, the final temperature is 32.8°C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

A 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is reached. The sample is quickly transferred to 55.604 g of water at 22.6°C contained in a calorimeter. When thermal equilibrium is reached the temperature of the water is measured to be 27.3°C. What is the specific heat of the metal? Specific heat of water is 4.184 J/ grams•°C   In part A, (metal-water ) how was the initial temperature of WATER determined?   In part A, (metal-water ) how was the initial temperature of METAL determined?

When 12.29 g of finely divided brass at 95.0 °C is quickly stirred into 40.00 g of water at 22.0 °C, the water temperature rises to 24.0 °C. Assuming heat can only transfer between the brass and the water, calculate the specific heat of brass. (Specific heat capacity of water is 4.18 J/g* oC)