5000 molecules are present in a sample hydrogen gas having a volume V at STP. Calculate the volume of nitrogen gas which has 2.5*10^8
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You can determine the volume of 3.0 x 1025molecules of Neon at STP using the ideal gas law : PV = nRT, solving for V. You must convert the molecules of Neon to moles using Avagadro's number, 6.022 x 1023. STP for gas laws is 0oCand 1 atm. You will need to convert the Celsius temperature to Kelvins, which is the temperature scale used in the gas laws.
Convert molecules of Neon to moles.
3.0 x 1025 molecules Ne x 1 mol Ne/6.022 x 1023molecules Ne = 49.82 moles Ne
(I'm leaving some guard units to reduce rounding errors.)
Given/Known:
P = 1 atm
n = 49.82 moles
R = 0.08205746 L atm K−1mol−1
T = 0oC+273.15=273.15K
Unknown:
Volume
Equation:
PV = nRT
Solution:
Divide both sides of the equation by P. Solve for V.
V = nRTP
V = 49.82 moles x 0.08205746 L atm K−1mol−1 x 273.15K/1 atm = 1100 L
(The answer is rounded to two scientifiction figures because 3.0 x 1025 has two significant figures.)
Answer:
The volume of 3.0 x 1025 molecules Ne at STP is 1100 L.
Convert molecules of Neon to moles.
3.0 x 1025 molecules Ne x 1 mol Ne/6.022 x 1023molecules Ne = 49.82 moles Ne
(I'm leaving some guard units to reduce rounding errors.)
Given/Known:
P = 1 atm
n = 49.82 moles
R = 0.08205746 L atm K−1mol−1
T = 0oC+273.15=273.15K
Unknown:
Volume
Equation:
PV = nRT
Solution:
Divide both sides of the equation by P. Solve for V.
V = nRTP
V = 49.82 moles x 0.08205746 L atm K−1mol−1 x 273.15K/1 atm = 1100 L
(The answer is rounded to two scientifiction figures because 3.0 x 1025 has two significant figures.)
Answer:
The volume of 3.0 x 1025 molecules Ne at STP is 1100 L.
ksaisumedhostlmk:
ohhk..But for hydrogen?
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