Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO,)MgO)+ CO,) AH-117.3 J (a) Is heat absorbed or released in the reaction? absorbed released (b) What is AH for the reverse reaction? kJ (e) What is AH when 5.20 mol of CO, reacts with excess Mg0? kJ (d) What is AH when 32.5 g of CO, reacts with excess Mg0? kJ

(3)

How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar?  The reaction we performed was:                   Na(s) + H2O(l)    NaOH(aq) + 1/2H2(g)                               qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is:                  0 = qsystem = qreaction + qwater    qreaction = -qwater                  qreaction = -mwater*Cwater*Twater The data from the demonstration was:  (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g How many moles of sodium were added to the water (in moles)?

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition:  2 H2O2 (l) --> 2H2O (l) + O2 (g) Delta H = -196.1 kJ Calculate the heat for the decomposition of 780. kg of H2O2.

Heat of reaction (AH°) for the following reaction at 25.0 °C is Fe;O4(6) + CO(g) 3FEO(s) + CO2(g) Given the following Heat of Formation: AHF0304(s) = (-1118 kJ/mol), AHCO(g) = (-110.5 kJ/mol), AHF«06) = (-272KJ/mol), AHco2(g) ( -393.5 kJ/mol),