In a bomb calorimeter compartment surrounded by 0.97 kg of water, the combustion of 1.298 g of benzene, C6H6 (I), raised the temperature of the water from 23.640°C to 32.692°C. The heat capacity of the calorimeter is 0.929 kJ/°C. What is AE for the reaction in kJ/mol of C6H6 (1), the specific heat of water is 4.184 J/gᵒC. Enter the correct sign (+ or -). Enter to O decimal places.

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?

When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.

A 1.615-g sample of benzoic acid, C7H6O2 (122.12 g/mol) was burned in a bomb calorimeter with excessoxygen. The temperature of the calorimeter and the water before combustion was 17.49 °C; after combustionthe calorimeter and the water had a temperature of 27.28 °C. The calorimeter had a heat capacity of 832 J/K,and contained 0.837 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of benzoicacid.

The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol

The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol

5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)

In an experiment, a 0.4481 g sample of 2-naphthylacetic acid ( C12H10 O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.290 10³ g of water. During the combustion the temperature increases from 28.40 to 30.68 °C. The heat capacity of water is × -1.°C-¹. 4.184 J The heat capacity of the calorimeter was determined in a previous experiment to be 928.7 J. C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 2-naphthylacetic acid based on these data. C12H10 O2 (s) + (27/2) O2(g) → 5H₂O(1) + 12CO2(g) + Energy kJ/mol e g Molar Heat of Combustion =