Given the following combustion reaction and its molar enthalpy of reaction: 2NO(g) + O2(g) 2NO2(g) AH° = -112 kJ What is the heat (q) associated with the combustion of 2.00 mole of NO(g)? O -112 kJ O -224 kJ +56.0 kJ -56.0 kJ O +112 kJ

Given that: AH°f [Ba(OH)2 (s)] =- 944.7 kJ/mol AH°F [Ba+2 (aq)] = - 537.6 kJ/mol AH°F [OH (aq)] = - 230.0 kJ/mol What is the enthalpy change for the precipitation reaction of Ba(OH)2 (s)? + 52.9 kJ/mol OA. O B.-1712.3 kJ/mol - 177.1 kJ/mol Oc-1 +360.5 kJ/mol D. - 227.5 kJ/mol OE.

33.9 Given the following two reactions and their enthalpy changes,             2 ClO2 (g)   -->   Cl2 (g)   +   2 O2 (g)                                      Delta H =  – 204 kJ             2 TiCl4 (l)   +   2 O2 (g)    -->    2 TiO2 (s)   +   4 Cl2                Delta H =  – 139.8 kJ What is the value of the enthalpy change for the reaction that is the sum of these two reactions?             2 ClO2 (g)   +  2 TiCl4 (l)    -->   2 TiO2 (s)   +   5 Cl2            Delta H =  ? Select one: a. – 64 kJ b. – 344 kJ c. 64.2 kJ d. 64 kJ e. 344 kJ f. – 204 kJ g. none of these

Calculate Δ­H for the reaction  NO(g) + O(g) → NO2(g) given the following information: NO(g) + O3(g) → NO2(g) + O2(g)                     Δ­H = -198.9 kJ O3(g) → 3/2O2                                                   Δ­H = -142.3 kJ                          O2(g) → 2 O(g)                                                   Δ­H = 495.0 kJ