The value of ka for nitrous acid (hno2) at 25 ∘c is 4.5*10-4. what is the value of δg at 25 ∘c when [h+] = 5.9*10-2m, [no2-] = 6.3*10-4m, and [hno2] = 0.21m? be sure to express your answer in units of kj in the box below. answers without units will not be given credit.

To get the value of ΔG we need to get first the value of ΔG°:

when ΔG° = - R*T*㏑K

when R is constant in KJ = 0.00831 KJ

T is the temperature in Kelvin = 25+273 = 298 K

and K is the equilibrium constant = 4.5 x 10^-4

so by substitution:

∴ ΔG° = - 0.00831 * 298 K * ㏑4.5 x 10^-4

= - 19 KJ

then, we can now get the value of ΔG when:

ΔG = ΔG° - RT*㏑[HNO2]/[H+][NO2]

when ΔG° = - 19 KJ

and R is constant in KJ = 0.00831

and T is the temperature in Kelvin = 298 K

and [HNO2] = 0.21 m & [H+] = 5.9 x 10^-2 & [NO2-] = 6.3 x 10^-4 m

so, by substitution:

ΔG = - 19 KJ - 0.00831 * 298K * ㏑ (0.21/5.9x10^-2*6.3 x10^-4)

= - 40