The energy change, q, for a system is given by the formula q=m * C * change T. C is the specific heat of the compound of interest and m is it's mass. If a 42.67 g of a compound is heated from 19.27 oC to 29.06 oC.What is the change in temperature?

An electrical heater is used to add 19.75 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter increases by 4.76°C. When 2.00 g of methanol (CH3OH) is burned in the same calorimeter, the temperature increases by 10.92°C. Calculate the molar heat of combustion for methanol (in kJ).

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.8608 g sample of glutaric acid (C3HgO4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.029x103 g of water. During the combustion the temperature increases from 25.01 to 27.84 °C. The heat capacity of water is 4.184 J gl°c-!. The heat capacity of the calorimeter was determined in a previous experiment to be 839.5 J°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of glutaric acid based on these data. C;HgO4(s) + 50,(g) 4 H,O(1) + 5 CO,(g) + Energy Molar Heat of Combustion = kJ/mol

A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = kJ What is the enthalpy of the reaction? AHrxn kJ/mol =

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.81kg sample of C4H6O2 from 31.4c to 49.6c. The experiment shows that 2.48*10^4 J of heat are needed. what can the chemist report for the molar heat capacity of C4H6O2 ? Round your answer to 2 sig figs.

NW113AACE04-21 3. a hunk of metal-like substance was found in an archeological site. In an attempt to identify it, the metal was heated and placed in a calorimeter containing water and determined the specific heat of the metal. If the specific heat of the metal is 0.448 J/g °C, what is the approximate molar mass (atomic mass) and likely identity of the metal? (Hint: compare the molar mass (atomic mass) of metal that of metals in periodic table)

When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?

A 79.1 g sample of an unknown solid is heated to 62.6ºC and placed into a calorimeter containing 92.1 g of water at 22ºC. If the final temperature of the solid sample and the water is 32.5ºC, what is the specific heat of the solid? Please provide your final answer rounded to two decimal places.

2. Slaked lime (Ca(OH)2(s)) is produced when lime (calcium oxide, Cao (s)) reacts with liquid water. 65.2 kJ of heat is released for each mol of Ca(OH)2 that is produced. (a) Write a thermochemical equation for the reaction. (b) What is the enthalpy change when 523.3 kg of lime reacts with excess water?

At constant volume, the heat of combustion of a particular compound, compound A, is −3046.0 kJ/mol.−3046.0 kJ/mol. When 1.753 g1.753 g of compound A (molar mass =112.07 g/mol)=112.07 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.475 ∘C.6.475 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?     Suppose a 3.771 g3.771 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.65 ∘C25.65 ∘C to 29.76 ∘C.29.76 ∘C. What is the heat of combustion per gram of compound B?