Assuming ideal behavior, how much pressure will 2.75 mol hydrogen gas exert on the walls of a 4.00 L container at 35.0ºC?
2 answers:
Answer:
The correct answer is option A.
Explanation:
Pressure of the gas = P =?
Volume of the container in which gas is placed, V= 4.00 L
Temperature of the gas = T = 35°C = 308.15 k
Moles of gas = N = 2.75 mol
Using ideal gas equation:
PV=nRT
P = 17.3931 atm ≈ 17.4 atm
The pressure of the gas in the container is 17.4 atm.
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Answer:
4.2 m
Explanation:
The energy (E) of the selector region of the spectrometer is:
E = v*B (equation 1)
Where v is the velocity, and B the magnetic field.
The force with which particle forms a curved path can be calculated by:
Where r is the radius of the particle, m is the mass, and q the electric charge. So:
For equation 1: v = E/B, so:
The two species will be separated by Δr = 0.42 mm
Δr = Δm*E/(q*B*B')
E/(q*B*B') = r/m
Δr = Δm*r/m
r = m*Δr/Δm
r is the large of curvature, m is the avarege mass = (28.0106 + 28.0134)/2 = 28.012:
r = (28.012*0.42)/(28.0134 - 28.0106)
r = 11.76504/(0.0028)
r = 4201.8 mm
r = 4.2 m