Question

At 3000 K and 1.000 atm, 83.00% of the oxygen molecules in a sample have dissociated to atomic oxygen. At what pressure will 92.00% of the molecules dissociate at this temperature? Pressure am

Answer 1

Here is the Solution:

The 83.0% of the oxygen molecules in sample have dissociated to atomic oxygen. O2(g) 20(a) First, we will calculate the number of moles of oxygen present in 83.0% of the oxygen molecule. 1 mol O2 6.023 x 1023 molecules Oz Number of moles of oxygen = 1.378 x 10-24 mol O2. Number of moles of oxygen = 100 % molechtes Ozxa Second, we will calculate the number of moles of oxygen present in 92.00% of the oxygen molecule. 1 mol O2 = 7000* molecules oz x ber of moles of oxygen - 92.00% -molecules O, X oa 1023 molecules Number of moles of oxygen = 1.527 x 10-24 mol Oy. Now, Using Avogadro's law, we can calculate the pressure of molecule. P1 P2 n nz We have, ni = Number of moles of oxygen in 83.0% = 1.378 x 10-24 mol n = Number of moles of oxygen in 92.00% = 1.527 x 10-24 mol P1 = 1.000 atm Pz = -----? 1.000 atm 1.378 x 10-24 mol 1.527 x 10-24 mol Pa = 1.108

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