These questions are all about indirect and direct variation with PV=nRT, the ideal gas equation
Q3. false, because of PV=nRT, the ideal gas equation if V goes up, P has to go down to equal nRT
Q4. false, if V remains constant, and P and T are constant as moles of gas are added, then something is wrong becse something has to change when stuff is added (V has to go down)
Q5. PV=nRT when T and n are constant, (R is the gas constant) PV=k, aka V=k/P which means inversly proportional
TRUE
Q6. ggeasy refer to past question PV=k if P is doubled then V has to halve in order to equal k 1/2 times 2=1 volume is halved
Q7. use charles law V/T=k so given V=4 T= kelvins, so 299 4/299=k so when temp goes to 22 does V go to 3.95 4/299=3.95/295? true because they're equal
Q8 FALSE, must be used in kelvins T=absolute tempurature in kelvins
Q9 PV=nRT solve for T (PV)/(nR)=T
use final volumes and pressures P=5atm V=24L n=1 R=0.082057 atm L/(mol K) (5atm*24L)/(1mol*0.082057 atm L/mol K)=T see, if you didn't mess up, the units cancel nicely T=1462.4 1200 K is closest
Q10 PV/T=constant because moles are constant (supposedly)
V=4L P=2.08atm T=275K
so find initial to final is constant (2.08atm*4L)/(275K)=(Pfinal*2.5L)/(323K) solve for Pfinal Pfinal=3.92315 atm answer is 3.9atm
In the absence of neap tide transect data this hypothesis cannot be tested directly, but three pieces of indirect evidence weigh against it as a complete explanation.
