Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: P4010(s)+6H2O (l) → 4HPO4(s) Round your answer to zero decimal places. 0 kJ ☐ x10 ×

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 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

Estimate ΔHrxn for the following reaction: C2H4+H2→C2H6 Give your answer in kJ per mole.

Consider the unbalanced equation for the neutralization of acetic acid: αHC2H3O2(aq)+βBa(OH)2(aq) →γH2O(l)+δBa(C2H3O2)2(aq) Balance the equation. Give your answer as an ordered set of numbers α, β, γ, δ. Your answers should reflect the lowest whole-number ratio of coefficients.

For a certain chemical reaction, the equilibrium constant  K   =   ×7.7106  at  5.00   °C . Calculate the standard Gibbs free energy of reaction.Round your answer to  2  significant digits.

Enter your answer in the provided box. Kf for the complex ion Ag(NH3)2+ is 1.5 × 107 at 25 ° C. Using this information, calculate the value of Δ G o   f for Ag(NH3)2+(aq).

What is the maximum amount of useful work that could possibly be obtained at 25 °C and 1 atm from the combustion of 47.9 g of natural gas, CH4(g), to give CO₂(g) and H₂O(g)? Express your answer as a positive value. kJ