Since you've got the first part, I'll just answer the second question, so to speak.
So, you've got your balanced chemical equation for this double replacement reaction
#AgNO_(3(aq)) + KCl_((aq)) -> AgCl_((s)) + KNO_(3(aq))#
You know that you have a #"1:1"# mole ratio between all the species involved. This means that the number of moles of potassium chloride must be equal to the number of moles of silver nitrate.
Since I assume you've calculated the number of moles of silver nitrate to be
#C = n/V => n = C * V#
#n_(AgNO_3) = "0.162 M" * "1.27 L" = "0.206 moles"# #AgNO_3#
automatically you'll have
#"0.206"cancel("moles "AgNO_3) * ("1 mole" KCl)/(cancel("1 mole "AgNO_3)) = "0.206 moles"# #KCl#
Now use the volume of potassium chloride given to figure out what the solution's concentration must be in order to have that many moles of #KCl# available for the reaction
#C = n/V = "0.206 moles KCl"/"3.78 L" = color(red)("0.0545 M")#