Ten moles of a gas are contained in a 1.00 L container at 295 K. What is the pressure of the gas?
1 Answer
Explanation:
We're asked to find the pressure of a gas, given its temperature, and volume, and number of moles.
We can use the idealgas equation:
#ul(PV = nRT#
where

#P# is the pressure of the gas (what we're trying to find) 
#V# is the volume occupied by the gas (given as#1.00# #"L"# 
#n# is the number of moles of gas present (given as#10# #"mol"# ) 
#R# is the universal gas constant, equal to#0.082057("L"·"atm")/("mol"·"K")# 
#T# is the absolute temperature of the gas (which must be in units of kelvin), given as#295# #"K"#
Let's rearrange the above equation to solve for the pressure,
#P = (nRT)/V#
Plugging in known values:
#color(red)(P) = ((10cancel("mol"))(0.082057(cancel("L")·"atm")/(cancel("mol")·cancel("K")))(295cancel("K")))/(1.00cancel("L")) = color(red)(ulbar(stackrel(" ")(" "242color(white)(l)"atm"" "))#
The pressure is thus