The equilibrium constant for a reaction is 0.48 at 25 °c. what is the value of δg° (kj/mol) at this temperature?
(a) 1.8
(b) -4.2
(c) 1.5 x 10^2
(d) 4.2
(e) more information is needed.

a) 1.8 kJ

Explanation:

ΔG=-RtLnK

Just input the data into the equation to gives us the result, in Joules.

ΔG=-8.314*(25+273.15)*ln(0.48)

ΔG=1819,37 J

But there is only 2 significant figures, so we express it as or 1.8 kJ

i think slash and

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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