How would you calculate the volume of 3.03 g of H2(g) at a pressure of 560 torr and temp of 139 k?
1 Answer
Explanation:
I would use the ideal gas law equation
#color(blue)(PV = nRT)#
and rearrange to solve for the volume of the gas,
#V = (nRT)/P" "# , where
Now, you have everything you need to calculate the volume of the gas except the number of moles.
To find how many moles of gas you have in that sample, use hydrogen's molar mass
#3.03color(red)(cancel(color(black)("g"))) * "1 mole H"_2/(1.00794color(red)(cancel(color(black)("g")))) = "3.006 moles H"_2#
Now plug in your values and solve for
#V = (3.006color(red)(cancel(color(black)("moles"))) * 0.082(color(red)(cancel(color(black)("atm"))) * "L")/(color(red)(cancel(color(black)("mol"))) * color(red)(cancel(color(black)("K")))) * 139color(red)(cancel(color(black)("K"))))/(560/760color(red)(cancel(color(black)("atm")))) = color(green)("47 L")#
The answer is rounded to two sig figs, the number of sig figs you gave for the pressure of the gas.