Question #e9ae8

1 Answer
Dec 11, 2016

(77.95" g")/"mole"77.95 gmole

Explanation:

Let R =R= The Gas Constant = 62.363=62.363 L Torr K"^-11 mole"^-11

Given: P = 400" torr"P=400 torr and T = 127" C"^@ = 400" "KT=127 C=400 K

The Ideal Gas law is:

PV = nRTPV=nRT

We are not given the volume but we do not need it; the reason will soon become obvious. Solve for the Volume per Moles:

V/n = (RT)/PVn=RTP

V/n = ((62.363" L Torr K"^-1" mole"^-1)(400" K"))/(400" Torr")Vn=(62.363 L Torr K1 mole1)(400 K)400 Torr

I am taking an extra step to show you that the Numbers for temperature and pressure cancel and and their units are canceled by the gas constant:

V/n = ((62.363" L "cancel("Torr")cancel(K^-1)" mole"^-1)(cancel(400)cancel(" K")))/(cancel(400)cancel(" Torr"))

No matter what Volume or number of moles we pick, at this temperature and pressure, the following ratio is true:

(62.363" L")/"mole" = V/n

We are given the mass density: (1.25" g")/"L"

To find the Molar Mass, we use the Factor-Label Method (a.k.a. Dimensional Analysis):

(1.25" g")/cancel("L")(62.363cancel(" L"))/"mole" = 77.95" g"/"mole"