A serving of Chocobits cereal is 122 g.A 1.00-g sample of the cereal is burned in a bomb calorimeter that has a heat capacity, C, of 8.50 kJ K-1, causing the temperature to increase from 25.0°C to 25.8°C. Calculate the energy of Chocobits in Calories per serving to three significant figures. 1 Cal = 4.184 kJ

If a 50.0g sample of Cu is heated to 180.00C and is placed in 100.0 ml of water in a calorimeter at 25.00C, what will the final temperature be for the system? Assume that all of the heat goes from the copper to the water. (None is lost to the surroundings or calorimeter.) dH20 =1.00g/ml C Cu = 0.385J/goC CH2O = 4.184 J/goC

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.

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.

1 Cal= 4.18 kJ

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.

If 0.067 mol of hydrochloric acid  (HCl)  is mixed with 0.067 mol of sodium hydroxide  (NaOH)  in a "coffee cup" calorimeter, the temperature of  5.1 g  of the resulting solution increases from 25.0 ° C to  34.0 ° C.   Given that  the energy released is    2.2  ×  101  cal when the specific heat of the resulting solution is  1.00 cal/g− ° C,  use a conversion factor to convert the energy released to joules (J). Enter your answer in scientific notation. Be sure to answer all parts.

When a 1.0 g sample of a candy bar is combusted in a bomb calorimeter whose total heat capacity (including the water) is 5.0 kJ/°C, the temperature of the water increases by 6.0 °C. If the candy bar has a mass of 28 g, calculate the total number of Calories that it contains. (1 Calorie = 103 calories, and 1 calorie = 4.184 J). Give your answer to the nearest 100 Calories, but not in scientific notation. Type your answer.

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 65.54 grams of copper to 98.08 °C and then drops it into a cup containing 78.67 grams of water at 23.78 °C. She measures the final temperature to be 29.26 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Specific Heat (Cu) = J/g°C.

A hot metal weighing 65.0 g was heated to 125 oC and dropped into 75.0 g of water kept at a room temperature of 20.6 oC in a calorimeter. Within a couple of minutes, water’s temperature increased to 26.8 oC and stayed constant at that temperature. If the heat capacity of calorimeter constant is 11.5 J/oC, find the specific heat capacity of the metal.