The change in enthalpy of combustion of 1 mole of thymol at 298.15 K is determined to be -5660 kJ at constant pressure. C10H14O(l) + 13 O2(g) → 10 CO2(g) + 7 H2O(l)

What is ΔE for this reaction at 298K?

The correct answer should be "electrons orbit the nucleus in circular motions exactly as shown on the classic bohr model."

Answer is: the equilibrium  shifts toward the reactants, to the left side of chemical reaction.it is because lead(ii) nitrate dissociates in water: pb(no₃)₂ → pb²⁺(aq) + 2no₃⁻(aq).according to lechatelier's principle, the position of equilibrium moves to counteract thechange (more lead cations, common ion), the position of equilibrium will move so that the concentration ofproducts decrease and concentration of reactants of chemical reaction increase.read more on -