3. Calculating pressure from Ko and equilibrium amounts (a) In the following reaction:
2NO2 (a)_] 2NO (g) + O2 (g)
at a temperature of 700K, the amount of each gas present at equilibrium is 0.96 mol of
NO2, 0.04 mol of NO and 0.02 mol of O2. If Ke = 6.8 x 10-6 atm what must the total
pressure have been to obtain this particular equilibrium mixture?
(b) Ke = 3.72 atm at 1000K for the system:
C (s) + H2O (g) 0 Có (g) + H2 (g)
What pressure must be applied to obtain a mixture containing 2.0 mol of CO,
1.0 mol of H2 and 4.0 mol of H2O?

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

if you need further assistance, let me know: )

~ trueboss72

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.

i think is conclusions.i think so