Question #12c2c
1 Answer
Explanation:
The idea here is that you're looking for the mass of the metal that will displace exactly
The first thing that you need to do here is to use the ideal gas law equation
#color(blue)(ul(color(black)(PV = nRT)))#
Here
#P# is the pressure of the gas#V# is the volume it occupies#n# is the number of moles of gas present in the sample#R# is the universal gas constant, equal to#0.0821("atm L")/("mol K")# #T# is the absolute temperature of the gas
to find the number of moles of hydrogen gas,
Rearrange the equation to solve for
#PV = nRT implies n = (PV)/(RT)#
Plug in your values to find
#n = (1 color(red)(cancel(color(black)("atm"))) * 1.12color(red)(cancel(color(black)("L"))))/(0.0821(color(red)(cancel(color(black)("atm"))) * color(red)(cancel(color(black)("L"))))/("mol" * color(red)(cancel(color(black)("K")))) * 293.15 color(red)(cancel(color(black)("K")))) = "0.04654 moles H"_2#
The number of moles of elemental hydrogen present in your sample will be equal to
#0.04654 color(red)(cancel(color(black)("moles H"_2))) * "2 moles H"/(1color(red)(cancel(color(black)("mole H"_2)))) ~~ "0.09308 moles H"#
Convert this to grams by using the molar mass of elemental hydrogen
#0.09308 color(red)(cancel(color(black)("moles H"))) * "1.008 g"/(1color(red)(cancel(color(black)("mole H")))) = "0.09382 g"#
Now, if
#1.008 color(red)(cancel(color(black)("g H"))) * "2.4 g metal"/(0.09382color(red)(cancel(color(black)("g H")))) = color(darkgreen)(ul(color(black)("26 g metal")))#
The answer is rounded to two sig figs, the number of significant figures you have for the mass of the metal.
SIDE NOTE I suspect that the problem was designed with the old STP conditions in mind, i.e. a pressure of
Under these conditions for pressure and temperature, the molar volume of an ideal gas is equal to
In this case, the number of moles of elemental hydrogen would come out to be equal to