If 1 10 liter sample of O2 gas at 300 kelvin and 0.5 atmosphere of pressure contains 5.0 x 10^22 molecules how many molecules would a 10 liter sample of H2 have if it was at the same temperature and pressure as the oxygen remember that hydrogens are 1/16th the size of oxygen

Explanation:

The detailed steps and calculations is as shown in the attached file.

 Number of molecules of H2=4.5454375x

Explanation

Given:

P1=P2=0.5 atmosphere=0.505xpa

T1=T2=300k

V1=10 liters of O2

N=5.0x 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=1.38XJ/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

N2=1.4545x5.0x =7.2727x molecules of O2

Recall that

N2 of H2=1/16 of N2 of O2

∵Number of molecules of H2=1/16 of 7.2727x

=4.5454x

Number of molecules of H2=4.5454375x

1 is the answer to this problem

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.