thermodynamics - Correlation between the equilibrium constant and delta G

I understand this up until the last two steps. How does $\ln(K_\mathrm{eq})$ become $2{,}303\log(K_\mathrm{eq})$ and how does $-RT\cdot2{,}303$ become $-1{,}42$?

Answer

How does ln(Keq) become 2,303log(Keq)

Because $e^{2.303} = 10$ and

$\ln(x) = \log (10^{\ln(x)})$ therefore

$\ln(x)=\log((e^{2.303})^{\ln(x)})$

$\ln(x)=\log (x^{2.303})$

$\ln(x)=2.303\log(x)$

how does -RT*2,303 become -1,42?

That would only be true at a particular temperature in a particular set of units