For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2 NO ( g ) + O 2 ( g ) − ⇀ ↽ − 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ G ° = − 69.0 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are P NO = 0.500 atm , P O 2 = 0.200 atm , and P NO 2 = 0.600 atm ?

The for the given reaction at 298 K is -64.11 kJ/mol

Explanation:

For the given chemical equation:

The equation used to Gibbs free energy of the reaction follows:

where,

= free energy of the reaction

= Standard Gibbs free energy = -69.0 kJ/mol = -69000 J/mol   (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314 J/K mol

T = Temperature = 298 K

= Ratio of partial pressure of products and reactants =

Putting values in above equation, we get:

Hence, the for the given reaction at 298 K is -64.11 kJ/mol

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

they are made of gases.

they have a spherical shape.

they make energy through fusion.