28.0g of a substance with a molecular weight of 52.0 g/mol is placed in a bomb2 calorimeter with a heat capacity of 2.60 J/°C and combusted. What is the molar heat of combustion for the substance if the temperature of the calorimeter went from 25.0°C to 142.0°C? Convert to J and Cal.

6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).

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

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)

when 50.0 mL of 0.200 M NaOH is mixed with 50 mL of 0.200 M HCl in a coffee cup calorimeter, the temperature increases from 23.5 degrees C to 26.5 degrees C. Assuming that the density of the resulting solution is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g degrees C, what is qrxn?

When a 0.740-g sample of trinitrotoluene (TNT), C,H,N,O, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter and its content is 3.35 kJ/°C. How much heat was produced by the combustion of the TNT sample? O 34.2 kJ O 11.7 kJ O 101.5 kJ

A student conducted several calorimetry investigations. In the first of the investigations, the student heats a 21.0 g price of metal that is know to have a specific heat capacity of 0.449 J/g°C to a temperature of 80°C. Then a piece of metal is added to the beaker of water (70.0 grams at 20.00°C). The specific heat capacity of water is 4.187 J/g°C. If the student repeated the investigation with 50.0 g of water instead what would be different.

When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature of the water rises from 21.6 to 37.8oC. Was the chemical reaction (dissolving the solid) endothermic or exothermic? How do you know? Write a balanced chemical equation for this process. Determine how many joules of heat (q) were involved in changing the temperature of the water. If the heat that changed the temperature of the water was a result of the chemical reaction, determine the ΔH of the chemical reaction in kJ/mol of sodium hydroxide.