Answer:
Explanation:
The detailed steps and calculations is as shown in the attached file.
Answer:
Number of molecules of H2=4.5454375x[tex]10^{21}[/tex]
Explanation
Given:
P1=P2=0.5 atmosphere=0.505x[tex]10^{5}[/tex]pa
T1=T2=300k
V1=10 liters of O2
N=5.0x[tex]10^{22}[/tex] molecules
10 liters of H2
V2=? liters of O2
H2=1/16 of O2
Procedure:
for every liter of H2, there are 16 liters of O2 since H2=1/16 of O2,
Therefore, 10 liters of H2= 160 liters of O2 i.e.
V2=160 liters of O2.
Applying ideal gas equation,
VP=NkT :where P is pressure, V is volume, N is number of molecules, T is temperature in kelvin and k is Boltzman constant=1.38X[tex]10^{-23}[/tex]J/K.
considering change in volume of O2, N can be calculated as follows:
V1P1=N1kT1..................................(1)
V2P2=N2kT2...............................(2)
dividing (2) by (1)
V2P2/V1P1=N2kT2/N1kT1
but P1=P2 and T1=T2 since they remain the same, they cancel out.
∵ V2/V1=N2/N1
substituting values, we have
160/110=N2/5.0x[tex]10^{22}[/tex]
N2=1.4545x5.0x[tex]10^{22}[/tex] =7.2727x[tex]10^{22}[/tex] molecules of O2
Recall that
N2 of H2=1/16 of N2 of O2
∵Number of molecules of H2=1/16 of 7.2727x[tex]10^{22}[/tex]
=4.5454x[tex]10^{21}[/tex]
Number of molecules of H2=4.5454375x[tex]10^{21}[/tex]
