ClONO2 is stable during the Antarctic winter, but quickly decomposes to form •ClO and •NO2 during the Antarctic summer. Explain why this is so.

A.) What is the heat of reaction, ΔH°? CO2(g) + H2O(l) à H2CO3(aq)   –20.2 kJ mol–1   –1379 kJ mol–1   –592 kJ mol–1 B.)  What is the average bond energy in CO2? CO2(g)          ΔH°f, = –393.5 kJ mol–1 CO(g)           ΔH°f, = –110.5 kJ mol–1 C(g)              ΔH°f, = +715 kJ mol–1        CO32–(aq)      ΔH°f, = –676.3 kJ mol–1 O(g)               ΔH°f, = +249.0 kJ mol–1   207 kJ mol–1   1607 kJ mol–1   804 kJ mol–1

26. When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200°C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. a) Write a balanced chemical equation for the equilibrium reaction. b) Use bond enthalpies to estimate the enthalpy change for the reaction. c) Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? d) In which direction will the equilibrium shift as the temperature increases above 200°C? Explain. e) Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? f) Why is the equilibrium not established at room temperature?

Calculate ΔH° for the reaction using the given bond dissociation energies.   CH4(g)+2O2(g)⟶CO2(g)+2H2O(g) Bond ΔH° (kJ/mol) O–OO–O 142 H–OH–O 459 C−HC−H 411 C=OC=O 799 O=OO=O 498 C–OC–O 358 What type of reaction is this?

Consider the following reaction: 3 C(s) + 4 H₂(g) →→ C3H8(g) Which of the following statements is correct about this reaction? Use the following reactions and thermodynamic data: Reaction: C3H8(g) + 5 O2(g) → 3 CO₂ (g) + 4H₂O C(s) + O₂(g) → CO₂(g) 2 H₂(g) + O₂(g) → 2H₂O(g) AG=-23.4 kJ AS >0 The reaction is non-spontaneous The reaction is spontaneous not enough information is given AS <0 AG rxn (kJ) -394.4 -457.1 k

Ozone, O3, is an important absorber of UV radiation in our atmosphere. Upon absorption of UV radiation, O3 dissociates into molecular oxygen, O2, and a free oxygen atom. The free oxygen atom can then join with another O2 molecule to create more ozone, which can in turn absorb more UV radiation. Alternatively, the free oxygen atom could join with O3 to create more O2. 2 O3(g)→ 3 O2(g) The reaction would have a _______ △S. A) positive B) negative C) zero D) can't determine from given information   Why? (pick one) A) The moles of gas increase B) The moles of gas decrease C) The moles of gas remain constant. D) The total moles of product are greater E) The total moles of reactant are greater. F) The number of moles are the same in reactants and products

Decide whether each of the following reactions is product or reactant-favored. Then, calculate the standard enthalpy change of the reaction in each case and draw an energy level diagram to represent it. a) The decomposition of ozone, O3, to oxygen molecules b) the decomposition of MgCO3 (s) to give MgO(s) and CO2(g)

22. Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong base) is always -55.90 kJ per mole of H2O formed, what is the concentration of a 65 mL sample of HCl if the enthalpy of neutralization for the reaction was found to be -5.38 kJ, assuming no heat is lost to the calorimeter?       0.96 M     1.48 M     1.60 M     0.38 M     4.63 M

Write a balanced chemical reaction for the combustion of glucose (C6H12O6).

a) Define the term average bond enthalpy. b) Determine a value for the hydrogenation of propene. Thank you!