Consider the following chemical reaction:   C6H6(l) + O2(g) --------------> CO2(g) + H2O(g)  Calculate the change in internal energy of the reaction for 2.80 g C6H6(l). The temperature is 25oC.   C=12.01 g/ mole and H = 1.008 g/mole  delta H's :   C6H6(l) = -345

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H,O(1) → ADP(aq) + HPO (aq) for which AGixn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.40 mM, and [HPO?-] = 5.0 mM. AGxn kJ/mol %3D Is the hydrolysis of ATP spontaneous under these conditions? O yes

For the reaction given below, AH --1516 kJ at 25"C und AS--432.8 J/K at 25°C, This reaction is spontaneous SiH,(g) + 2 0:(g) SiO;()+2 H,0(6)

Consider the following reaction: 2 H2(g) + 2 NO(g) N2(g) + 2 H20(g) and the following table of standard enthalpies of formation and standard absolute entropies: compound AH (kJ mol-1) s° (J K-1 mol-1) H2(g) 130.8 NO(g) 91.3 210.8 N2(g) 191.6 H20(g) -241.8 188.8

Consider this reaction: C6H12O6 + 602 à 6CO2 + 6H₂O. What is the standard enthalpy AH°rxn given the standard molar enthalpies of the substances below? Substance C6H12O6 02 CO₂ H₂O AHᵒf (kJ/mol) -1274.4 0 -393.45 -241.8

8) Kirchhoff's Law Calculate the reaction enthalpy for the following reaction (ARH° = - 282.98 kJ mol¹¹) at a temperature of 400 °C: CO+0.502 → CO₂ In your calculations, consider the temperature-dependency of the molar heat capacities as follows: Cp (CO) = (21.75 +0.064 T-4.1.10-5T2)Jmol-¹K-1 Cp(O2) = (27.96 +0.004 T-1.7 10-7T²)Jmol¯¹K−¹ Cp (CO2)=(27.63 +0.005 T)Jmol-1K-1

Calculate the standard enthalpy change for the reaction at 25 ∘25 ∘C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl2(s)+H2O(l)⟶MgO(s)+2HCl(g)MgCl2(s)+H2O(l)⟶MgO(s)+2HCl(g) ΔH∘rxn=