The chemical reaction that causes aluminum to corrode in air is given by 4Al+3O2→2Al2O3 in which at 298 K   ΔH∘rxnΔHrxn∘ = −3352 kJ= −3352 kJ ΔS∘rxnΔSrxn∘ = −625.1 J/K   What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K.

For a certain chemical reaction, the standard Gibbs free energy of reaction is - 104. kJ. Calculate the temperature at which the equilibrium constant K = 7.1 × 10¹8. Round your answer to the nearest degree. T = °C X S

For a certain chemical reaction, the standard Gibbs free energy of reaction is  129.   kJ . Calculate the temperature at which the equilibrium constant K   =   ×6.010−25 .Round your answer to the nearest degree.

Calculate the standard entropy, Δ?∘rxn,ΔSrxn∘, of the reaction at 25.0 ∘C25.0 ∘C using the table of thermodynamic properties.   3C2H2(g)⟶C6H6(l)   Δ?∘rxn=   kJ⋅mol−1. Calculate the standard Gibbs free energy of the reaction, Δ?∘rxn. The standard enthalpy of the reaction, Δ?∘rxn, is −633.1 kJ⋅mol−1. Δ?∘rxn=    kJ⋅mol−1  Determine in which direction the reaction is spontaneous as written at 25.0 ∘C25.0 ∘C and standard pressure. forward reverse both neither

Suppose we redefine the standard state as P=4bar. Find the new standard ΔfG∘ values of the following substances.     Part A HCl (g)(ΔfG∘at1bar=−95.3kJmol−1)

For a certain chemical reaction, the equilibrium constant K = 2.8 × 104 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. Round your answer to 2 significant digits. AG° = kJ x10 X Ś

For a certain chemical reaction, the standard Gibbs free energy of reaction at 10.0 °C is 135. kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K= |

Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3 NO₂(g) + H₂O(1) AGixn || - 2 HNO3 (1) + NO(g) kJ/mol

A 0.588 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.706 kJ °C-1. If the temperature inside the calorimeter increased from 25.0 °C to 29.9 °C, determine ΔrU for this reaction in kJ mol-1 (with respect to C5H12). Do not worry about how realistic the final answer is. Express answer in 2 significant figures.

Determine the molar ΔH°solution for a soluble ionic compound when the dissolution of 0.171 moles of that compound leads to a 12.9 °C temperature increase in a constant pressure calorimeter. The heat capacity of the calorimeter is 1.120 kJ/℃.