A 26.0 g sample of acetylene,C2H2, is burned in a bomb calorimeter in which a change in temperature of 4.79 °C is observed. If the heat capacity of the calorimeter is 1.08 kJ/°C, what is the enthalpy of combustion () of acetylene?

A scientist measures the standard enthalpy change for the following reaction to be 209.4 kJ : CHĄ(g) + H20(g)3H2(g) + CO(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CH4(g) is kJ/mol.

When 0.0901 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter increases in temperature by 2.19°C. If the heat capacity of the bomb calorimeter is 1.229 kJ/°C, what is the heat of combustion for the unknown hydrocarbon?

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 2.30 g sample of ethanol, CH3CH2OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 4.89 K. If the heat capacity of the bomb is 663 J/K and it contains 2.57 kg of water, what is the enthalpy change per mole of ethanol combusted? The specific heat capacity of water is 4.18 J/g×K and the molar mass of ethanol is 46.07 g/mol.

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.

When 6.10 g of urea,(NH2)2CO (g), burns to produce CO2 (g), N2 (g) and H2O (l) 67.8 kJ of heat energy are released in a bomb calorimeter.  What is the energy released in the burning of one mole of urea?  Using this, what is the enthalpy of formation of urea?

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

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)