The answer is X Ray
Hope it helps
The standard formation equation for glucose C6H12O6(s) that corresponds to the standard enthalpy of formation or enthalpy change ΔH°f = -1273.3 kJ/mol is
C(s) + H2(g) + O2(g) → C6H12O6(s)
and the balanced chemical equation is
6C(s) + 6H2(g) + 3O2(g) → C6H12O6(s)
Using the equation for the standard enthalpy change of formation
ΔHoreaction = ∑ΔHof(products)−∑ΔHof(Reactants)
ΔHoreaction = ΔHfo[C6H12O6(s)] - {ΔHfo[C(s, graphite) + ΔHfo[H2(g)] + ΔHfo[O2(g)]}
C(s), H2(g), and O2(g) each have a standard enthalpy of formation equal to 0 since they are in their most stable forms:
ΔHoreaction = [1*-1273.3] - [(6*0) + (6*0) + (3*0)]
= -1273.3 - (0 + 0 + 0)
= -1273.3
Ionic bonds form when a nonmetal and a metal exchange electrons, while covalent bonds form when electrons are shared between two nonmetals. An ionic bond is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions.
Hope this helps!
Answer:
Reaction A and B are unfavorable.
Explanation:
Gibbs free energy is an energy which that can be use to convert into useful work.
ΔG°=ΔH°-TΔS°
ΔG°= Gibbs free energy
ΔH° = enthalpy of reaction
T = temperature of eh reaction
ΔS° = Entropy change
- If the Gibbs free energy of the reaction is positive than the reaction will be non spontaneous and the chemical reaction will be not feasible.
- If the Gibbs free energy of the reaction is negative than the reaction will be spontaneous and the chemical reaction will be feasible .
According to given information in the question:
Reaction A and B are non spontaneous as their Gibbs free energy value is positive.hence both are unfavorable.
