Consider the following reaction: 2NO(g)+O2(g)→2NO2(g)
Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.) I need to find the temperature are 298K and 702K. For 298K It is simple because at standard temperature
ΔG∘ = DG(products)- DG(reactants).

A. ; as such the reaction is said to be spontaneous since the value of is negative.

B.   and the reaction is spontaneous

Explanation:

The equation for this chemical reaction is :

Using the following relation to calculate ;

At 298 K; the standard Gibbs Free Energy for the formation are as follows:

Replacing them into the above equation;

Thus; ; as such the reaction is said to be spontaneous since the value of is negative.

B.

Using the same above chemical equation;

The relation used for calculating of the reaction when the temperature is 702 K is:

where;

Gibbs free energy of the reaction at 702 K

= standard enthalpy of the reaction = -116.2 kJ/mol

= standard entropy of the reaction = -146.6 J/mol/K

Temperature T = 702 K

Thus and the reaction is spontaneous

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.