Question #d9848
1 Answer
Explanation:
The ideal gas law states
ul(PV = nRT
where
-
P is the pressure (in"atm" ) of the gas -
V is the volume (in"L" ) the gas occupies -
n is the quantity (in"mol" ) of gas present -
R is the universal gas constant, equal to0.082057("L"·"atm")/("mol"·"K") -
T is the absolute temperature (in"K" ) of the gas (absolute temperature indicates units of Kelvin)
Standard temperature and pressure (STP) conditions are commonly used in chemistry as
-
ul(273.15color(white)(l)"K" -
ul(1color(white)(l)"atm"
(Standard pressure, since the year 1982, has been defined as
1 "bar" (0.9869 "atm" ), but a lot of instructors teach it as1 "atm" . The difference is small, but can cause differing calculations, so be sure to know which standard pressure you are to be using.)
Plugging these and the constant
(1color(white)(l)"atm")(V) = n(0.082057("L"·"atm")/("mol"·"K"))(273.15color(white)(l)"K")
We're asked to use the gas law to find the moles (
(1)(V) = (22.41)(n)
color(red)(ulbar(|stackrel(" ")(" "n = V/22.41" ")|)
Does the number