In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy change of a solution phase reaction. A student heats 62.57 g zinc to 98.12 °C and carefully lowers it into a cup containing 76.20 g water at 23.18 °C. She measures the final temperature to be 28.30 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.79 J/°C. Assuming that there is no heating of the surroundings calculate the specific heat capacity of zinc. Specific Heat (Zn) =  J g-1 °C-1.

A 30.0 g sample of chromium is heated to 100.0 °C in a boiling water bath. The sample is added to a calorimeter charged with 45.0 mL of water at 34.1 °C. The final temperature of the calorimeter contents is 38.5 °C. Calculate the specific heat of chromium.

A calorimeter is calibrated to have a heat capacity of 441.2 J/°c. 0.143 g of substance X is burned in the calorimeter and raises its temperature from 23.1 °c to 39.5°c. What is the heat of combustion of substance X in J/g?

A particular sample of cold graphite at 10.20 °C was added to 988.5 g of water at 25.31 °C in a constant pressure calorimeter. If the final temperature of the graphite and water was 25.17 °C, what was the mass of the graphite sample? Assume no heat was lost to the surroundings. The specific heat for water is 4.184 J/g•°C and the specific heat for this graphite is 0.7069 J/g•°C.

When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175.0 g of water was placed in a coffee-cup calorimeter and chilled to 10.0 °C. Then 49.0 g of pure sulfuric acid, also at 10.0 °C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9 °C. Assume that the specific heat capacity of the resulting sulfuric acid solution is 4.19 J/g °C. Calculate the quantity of thermal energy transferred, Q, for the formation of this solution, and calculate the molar enthalpy of solution in kilojoules per mole of H₂SO4.

10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C

Calculate the heat of reaction (in J)

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

n 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 63.03 grams of chromium to 98.03 °C and then drops it into a cup containing 79.71 grams of water at 23.19 °C. She measures the final temperature to be 28.85 °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 chromium.   Specific Heat (Cr) =  ____________J/g °C.

1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?