The complete combustion of  1.05 g of cinnamaldehyde (C9H8O, one of the compounds in cinnamon) in a bomb calorimeter (Ccalorimeter =  3.60 kJ/°C) produced an increase in temperature of  11.4 °C.   Calculate the molar enthalpy of combustion of cinnamaldehyde (ΔHcomb) (in kilojoules per mole of cinnamaldehyde).

The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d = 0.688 g/mL).

Suppose you burned 0.300 g of C(s) in an excess of O₂ (g) in a constant-volume calorimeter to give CO₂ (g). C(s) + O₂(g) → CO₂ (g) The temperature of the calorimeter, which contained 776 g of water, increased from 24.90 °C to 27.28 °C. The heat capacity of the bomb is 896 J/K. Calculate AU per mole of carbon. (The specific heat capacity of liquid water is 4.184 J/g. K.) AU = = kJ/mol C

Determine the molar enthalpy of combustion of an unknown fuel if a 2.75 g sample increased the temperature of 5.00 x 10° ml of hot chocolate (c = 3.75 J/g.°C) from 10 °C to 65.00 °C. The density of hot chocolate is 1.08 g/ml and the molar mass of the fuel is 44.10g/mol

A 3.59°C increase in temperature occurs when a 0.232 g sample of benzoic acid (C7H6O2) is combusted in a bomb calorimeter. A 1.81 °C increase in temperature occurs when a 0.303 g sample of citric acid (C6H8O7) is combusted in the same bomb calorimeter. The heat of combustion of benzoic acid is -26.37 kJ/g. What is the molar heat of combustion of citric acid? Reminder: Any heats of combustion will be negative since these are exothermic reactions.

Write a balanced equation for the reaction between gaseous methane (CH4)(CH4) and fluorine gas to produce gaseous carbon tetrafluoride and gaseous hydrogen fluoride. Include phases. balanced equation:   Calculate the standard enthalpy of reaction (Δ?∘rxn).(Δ⁢Hrxn∘). Use the standard enthalpy of formation values in this table of thermodynamic properties. For carbon tetrafluoride, use Δ?∘f=−933.2 kJ/mol.Δ⁢Hf∘=−933.2 kJ/mol. Δ?∘rxn=Δ⁢Hrxn∘=   Suppose that 0.433 mol0.433 mol of methane gas is reacted with 0.904 mol0.904 mol of fluorine gas. Assuming the reaction occurs at constant pressure, how much heat is released? amount of heat released:

The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5  × 104 kJ of heat?                                            2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ

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

When 9.42 g of methane (CH4) is burned in a bomb calorimeter (heat capacity = 2.677 × 103 J/°C), the temperature rises from 24.00 to 27.08°C.  Calculate the enthalpy change for the following reaction.  (C= 12.00 amu, H = 1.00 amu)                                                       CH4(g) + 2O2(g)  →  CO2(g) + 2H2O(l) Group of answer choices a. 8.425 kJ b. –14.01 kJ c. –8.425 kJ d. 8245 J e. 14.00 kJ

The combustion of 0.1556 g benzoic acid increases the temperature of a bomb calorimeter by 2.50°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 8 A 0.2194-g sample of vanillin (Cg H8O3) is then burned in the same calorimeter, and the temperature increases by 3.20°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol