ASAPStep by step having some trouble solving this

Question

A given sample of gas has a volume of 4.20 L at 60 deg * C and standard pressure. Calculate its 70 / (27 deg) * C pressure, in atm, if the volume is changed to 5.00 L and the temperature . What we know

v1=

p1=

t1=

v2=

P2=

t2=

Answer 1

The final volume (5.00 L) is greater than the initial volume (4.20 L). Since pressure decreases when volume increases (an indirect relationship exists between Pressure and Volume--Boyles"s Law). So, the net effect of changing the volume is that the original pressure of 1.00 atmosphere (Standard Pressure) will decrease when the volume increases.

Similarly, the final temperature (300 K) is less than the initial temperature (333 K). Since there is a direct relationship between gas pressure and absolute (Kelvin) temperature (Gay-Lussac's Law), the effect of decreasing the temperature is to decrease the volume.

Combining these two effects of changing volume and absolute temperature (the Combined Gas Law),

(1.00 atm.) (4.20 L)/5.00 L) (300 K)/333 K) = 0.757 atm