Asked by zhalia moon
Calculate the volume occuiped by 7g of nitrogen gas at 27degree centigrade and 750 mm of Hg pressure?
Answers
Answered by
Jai
assuming the gas is ideal, we can use the ideal gas law:
PV = nRT
where
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = gas constant = 0.0821 L-atm/mol-K
T = temperature (in K)
note that n = mass given / molar mass. The molar mass of nitrogen (diatomic gas) is equal to 28 g/mol. Also, K = C + 273 and 1 atm = 760 mm Hg.
substituting,
(750/760)*(V) = (7/28)*(0.0821)*(27+273)
now solve for V. units in liters.
hope this helps~ :)
PV = nRT
where
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = gas constant = 0.0821 L-atm/mol-K
T = temperature (in K)
note that n = mass given / molar mass. The molar mass of nitrogen (diatomic gas) is equal to 28 g/mol. Also, K = C + 273 and 1 atm = 760 mm Hg.
substituting,
(750/760)*(V) = (7/28)*(0.0821)*(27+273)
now solve for V. units in liters.
hope this helps~ :)
Answered by
Anonymous
7.8litres
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.