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 to#0.082057("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 as#1# #"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