How many moles of helium gas would it take to fill a balloon with a volume of 1000.0 cm^3 when the temp is 32 degrees C and the atmospheric pressure is 752 mm Hg
760mm Hg/1atm
Convert temperature to celsius.
convert pressure to atmospheres.
convert volume to liters.
R=> gas constant.
use PV=nRT
P= pressure
V= volume
n= moles of gas
R= gas constant
T= temperature
PV = nRT
T in Kelvin.
P in atmospheres = 752/760
yes but the reason is the conversion factor is what I posted below Dr.Bob's comment to clarify on that.
thus
mmHg(760atm/mmHg)= atm
forget ABOVE....
CORECTION:
mmHg(1atm/760mmHg)= atm
and the answer is =760
No, of course not. Use
PV = nRT to solve the problem.
You have pressure BUT it must be converted to atmospheres. The way to do that is to divide 752 by 760. That number, then you substitute for P in the formula. Likewise, substitute the other numbers for the remaining parameters to solve for the n, the number of mols.
how do you mix stuff
no, and I hope the anonymous person is not being mean..
What I posted above was the conversion for one part of the question, jerson.
you convert the pressure (how I did it above, but using the numbers you have in the problem)
Analyzing your problem because it seems you don't understand below:
How many moles of helium gas would it take to fill a balloon with a volume of 1000.0 cm^3 when the temp is 32 degrees C and the atmospheric pressure is 752 mm Hg
your given,
Volume= 1000.0cm^3
Temperature= 32oC
Pressure= 752 mmHg
m= ?
R= 8.314472
PV=nRT
so the problem is that you need the same information but converted into other units, specifically
The above units need to be converted to:
Volume= L (noting 1cm^3= 1ml)
Temperature= Kelvin (noting C= K-273.15)
Pressure= 752 mmHg (noting 1atm= 760mmHg)
R= 8.314472
n=? (your looking for this)
PV=nRT
n= moles
rearranged equation is:
n=PV/RT
and AFTER you convert the numbers given to you in the question, plug them into the equation and solve for moles(I rearranged the equation for you already)
if you need help POST YOUR WORK