What is the change in enthalpy in kilojoules when 3.24 g of CH3OH gas is completely reacted according to the following reaction? 2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ∆H = 252.8 kJ

Sucrose is common sugar. It is produced naturally in plants, from which table sugar is refined. A sample of sucrose (C12H22O11) with a mass of 2.68 g is burned in a bomb calorimeter. The heat capacity of this calorimeter is 8.91 kJ/°C. The temperature changes from 23.0°C to 30.5°C. Calculate the heat of combustion of sucrose in kilojoules per mole.     Question options: a. -8.54 x 103 b. 4.64 x 105 c. 2.01x 10-4 d. -1.88 x 102

The enthalpy of reaction for the formation of 2.00-mol ozone from 3.00-mol O2 (g): 3 O2 (g) à 2 O3 (g)  is ∆Horxn = 429 kJ at 1 atm and 25 oC. In this question, O2 (g) and O3(g) are rigid molecules and have the ideal gas behavior. Their molar heat capacities at constant pressure are independent of temperature, and follow the values shown in our lecture note (Page 56 in Chapter 2 Part 1). At -35 oC, the enthalpy of reaction for the above reaction ( 3 O2 (g) à 2 O3 (g) ) should be _______ 429 kJ.     Insufficient information     equal to         greater than       less than

The combustion of toluene has a AErxn of -3.91 x 10³ kJ/mol. When 1.30 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 22.80 °C to 36.11 °C. Find the heat capacity of the bomb calorimeter. Express your answer using three significant figures. Ccal = 17| ΑΣΦ ? kJ/°C

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 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol

Determine the amount of heat (in kJ) given off when 2.56 g of NO2 is produced according to the following equation: 2NO(g) + O2(g) → 2NO2(g)          ΔH = −114.6 kJ/mol Group of answer choices 3.19 kJ 5.56 kJ 6.38 kJ 1.14 kJ 114.6 kJ

The complete combustion of  1.35 g of cinnamaldehyde (C9H8O, one of the compounds in cinnamon) in a bomb calorimeter (Ccalorimeter =  3.10 kJ/°C) produced an increase in temperature of  13.4 °C.