I need some explaining. Easy question.?!
The mass of an evacuated 255mL flask is 143!.187g!. The mass of the flask filled with 267torr of an unknown gas at 25 degrees C is 143!.289g!. Calculate the molar mass of the unknown gas!.
Easy right!?
Using Ideal Gas Law I can find the number of mol!.
n = ( 0!.0821 L*atm / K*mol ) * ( 298K ) / ( 255mL * 1L / 1000mL ) * ( 267torr * 1atm / 760torr )
n = 273mol
g = 143!.289 - 143!.187
g = 0!.102
Now here's where I get messed up and I know it's something small I'm not seeing!. Molar Mass is ( g / mol ), so why in questions like this do I calculate it by doing ( mol / g ) * ( g / mol )!? Why is the solution not 0!.102 / 273!?Www@FoodAQ@Com
Easy right!?
Using Ideal Gas Law I can find the number of mol!.
n = ( 0!.0821 L*atm / K*mol ) * ( 298K ) / ( 255mL * 1L / 1000mL ) * ( 267torr * 1atm / 760torr )
n = 273mol
g = 143!.289 - 143!.187
g = 0!.102
Now here's where I get messed up and I know it's something small I'm not seeing!. Molar Mass is ( g / mol ), so why in questions like this do I calculate it by doing ( mol / g ) * ( g / mol )!? Why is the solution not 0!.102 / 273!?Www@FoodAQ@Com
Answers:
As already pointed out, wrong section!.
Maybe delete the question and put it in the correct section if you haven't figured it out yet!.Www@FoodAQ@Com
Maybe delete the question and put it in the correct section if you haven't figured it out yet!.Www@FoodAQ@Com
do people still know how to put the question in the right category!?Www@FoodAQ@Com
Uhhh!?!?!? what!?!?
Www@FoodAQ@Com
Www@FoodAQ@Com