Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: 2Al(s) + Fe₂O3 (s) → Al₂O3 (s) + 2Fe (s) Round your answer to zero decimal places. 8⁰0 X

Use this information to complete the table below.

Acetone, CH3 OCOCH3, is a fragrant liquid that is used as a solvent for lacquers, paint removers, and nail polish remover. It burns in oxygen to give carbon dioxide and water CH: COCH, (1) + 402 (9) → 3CO2(9) + 3H2O(1) If the standard free-energy change for this reaction is –1739.0 kJ/mol, what is the standard free energy of formation of acetone? Substance AG; (kJ/mol) O2 (9) Co (9) НаО() -394.4 -237.1 Standard free energy= kJ/mol

A student dissolves 11.8 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 20.0 °C to 33.6 °C over the course of 8 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH (ag) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NaOH. O…

A student determines the value of the equilibrium constant to be 2.30 x 10¹6 for the following reaction. Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1) Based on this value of Keq AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.57 moles of Ca(OH)2 (aq) at standard conditions at 298 K. AGO rxn kJ

Calculate the standard change in Gibbs free energy, AGixn, for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. KCI(s) K+ (aq) + Cl(aq) AGxn= Determine the concentration of K+ (aq) if the change in Gibbs free energy, AGran, for the reaction is -8.21 kJ/mol. [K+] = kJ/mol M

Consider the following reaction; A(g) + B(g) → c(s) + D(g); AH = 159.1 kJ; AG = 164.1kJ at 298 K %3D The reaction is spontaneous at relatively high temperatures only The reaction is spontaneous at all temperatures The reaction is nonspontaneous at all temperatures. The reaction is at equilibrium at 298 K The reaction is spontaneous at relatively low temperatures only

A student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K.     G°rxn =  ____kJ

Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation of NH3 (g) is -104 kJ/mol at 298 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

determine whether each reaction is spontaneous under standard conditions. If a reaction is not spontaneous, write the corresponding spontaneous reaction. K2O2 (s) → 2K (s) + O2(g) PbCO3 (s) → PbO (s) + CO2 (g) P4 (s) + 6H2(g) → 4PH3 (g) 2AgCl (s) + H2S (g) → Ag2S (s) + 2HCl (g)