This one is easy. It's just addition and subtraction. Add the partial pressure of Argon and the partial pressure of Helium:
152 kPa
<u>+305 kPa</u><u>
</u> 457 kPa
Next, subtract the result from the total pressure:
1015 kPa
<u>- 457 kPa</u>
558 kPa
Answer:
Explanation:
The neutral one has atomic structure 1s2 2s2
The one with a positive charge could be 1s2 2s which has lost one of its 2s electrons.
Answer:
Equilibrium constant Kc for the reaction will be 1.722
Explanation:
O2(g)+NO(g)→CO(g)+ NO2(g)
0.88 3.9 --- ---
0.88x 3.9-x x x
GIVEN:
0.88X-X= 0.11
⇒ X=0.77
CO2(g)+NO(g) → CO(g) + NO2(g)
0.88 3.9 --- ---
0.88-x 3.9-x x x
= 3.13 0.77 0.77
=0.11
Kc = ![\frac{[CO] *[NO2]} {[CO2]*[NO]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BCO%5D%20%2A%5BNO2%5D%7D%20%7B%5BCO2%5D%2A%5BNO%5D%7D%20)
=
= 1.722