Answer
24.4 L
Work Step by Step
$n= 20.2\,g\,NH_{3}\times\frac{1\,mol\,NH_{3}}{17.031\,g\,NH_{3}}=1.186\,mol$
$T= (-25+273)\,K=248\,K$
$R=0.08206\,atm\,L\,mol^{-1}K^{-1}$
$P=752\,mmHg\times\frac{1\,atm}{760\, mmHg}$
$=0.98947\,atm$
Using the ideal gas law, we have
$V=\frac{nRT}{P}=\frac{1.186\,mol\times0.08206\,atm\,L\,mol^{-1}K^{-1}\times248\,K}{0.98947\,atm}$
$=24.4\,L$