In the 1980s, there was an international agreement to destroy all stockpiles of mustard gas, ClCH2CH2SCH2CH2Cl. When this substance contacts the moisture in eyes, nasal passages, and skin, the -OH groups of water replace the Cl atoms and create high local concentrations of hydrochloric acid, which cause severe blistering and tissue destruction. Write a balanced equation for this reaction, and calculate ∆Horxn.

Determine the amount of heat (in kl) given off when 1.26 x 10'g of NO, ( Molar mass» 46 g/mole) are produced according to the equation: 2NO(s) 0,(s) > 2NO, (R) AH 114.6 kl/mol

7.312 g of dry ice (solid carbon dioxide) is placed in a sealed 2.000 L bag in a room where the pressure is 0.9140 atm. The carbon dioxide sublimes into a gas, and the bag expands to 12.116 L. If the enthalpy of sublimation for CO, is 25.9 kJ/mol, what is the total energy change of the system in kilojoules?

The combustion of 0.1587 g benzoic acid increases the temperature of a bomb calorimeter by 2.57°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 0.2140-g sample of vanillin (CHO3) is then burned in the same calorimeter, and the temperature increases by 3.25°C. What is the energy of combustion per gram of vanillin? Energy= kJ/g %3D Per mole of vanillin? Energy = kJ/mol %3D

Na(s) + ½ Cl2(g)   ¾®   NaCl(s)                       H°rxn =  –411.12 kJ/mol If 1.00 kg of sodium chloride is converted into solid sodium and chlorine gas through some industrial process, what will be the change in H°?

Determine the standard enthalpy (ΔH) for this reaction and explain the cooling effect that is experienced when methanol is accidentally dropped on the skin. The standard enthalpy of formation for CH3OH(l) is -239.1 kJ/mol and for CH3OH(g) is -189.83 kJ/mol. CH3OH(l) → CH3OH(g)

When 0.514 g of biphenyl, C12H10, undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 C to 29.4 C. Find ∆Urxn for the combustion of biphenyl. The bomb calorimeter contains 750.0 mL of water and has a heat capacity of 2.72 kJ/C.

A chemical reaction takes place in an open flask. The reaction releases 355 kJ of heat and does 25 kJ of work on the surroundings. Is the reaction endothermic or exothermic? Calculate ΔH for the reaction. Calculate ΔU for the reaction.

Consider the following chemical reaction which produces nitric oxide from its constituent elements: N2 (g) + O2 (g) → 2 NO (g) ArH= 182.6 kJ/mol If nitrogen and oxygen were mixed and allowed to react under constant pressure conditions, which of the following statements must be true? Select as many answers as applicable however points will be deducted for incorrect guesses. The temperature of the surroundings would increase This is an endothermic reaction ΔΗ = ΔU The temperature of the surroundings would decrease ΔΗ = q

Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.634 °C. Given the ∆H (-3069. kJ/mol) for the combustion reaction and the balanced chemical equation: C₅H₈ (l) + 7 O₂ (g) → 5 CO₂ (g) + 4 H₂O (g) Using the table below and the balanced chemical equation, determine the enthalpy of formation for C₅H₈, in kJ/mol.